pH

Topic Page

Questions

• How do you determine pH from pKa?
• How do pH values of acids and bases differ?
• How do you calculate something on a pH scale?
• How do you calculate pH diprotic acid?
• How do you calculate pH from acid dissociation constant?
• How do you calculate pH of acid and base solution?
• Why is the pH scale 0-14?
• Is pH a measure of the hydrogen ion concentration?
• How does solubility affect pH?
• How does pH relate to pKa in a titration?
• How can I calculate pH of NaOH?
• How do you calculate the pH of HCl?
• How does pH relate to molarity?
• How does pH differ from pOH?
• How does pH relate to H+ concentration?
• How does pH relate to concentration?
• How does pH change with depth?
• How does pH change protein structure?
• How does pH affect solubility?
• How does pH affect protein structure?
• How does pH affect photosynthesis?
• How does pH affect cellular respiration?
• How do you calculate the pH of a solution when given the OH- concentration?
• How do you calculate the pH of a weak acid?
• How do you calculate the pH of a buffer solution?
• What are some common mistakes students make with pH?
• What is an example of a pH practice problem?
• What are acid and base dissociation constants?
• Question #e4315
• Question #d8f04
• Question #b267a
• Question #6e2b5
• Question #7c902
• Question #7c9bd
• Question #3304e
• Question #091ee
• Question #4af57
• What is the concentration of the predominant form of #"H"_3"A"# at pH 10.5?
• Question #4bb1b
• Question #cbd61
• Question #9c4f9
• Question #d1234
• Question #d138d
• Question #46acb
• What are the initial pH and the pH at the equivalence if 0.2000 M acetic acid is titrated with 30.41 mL of 0.2000 M NaOH solution? Ka = 1.75 *10(-5)
• 47.25 mL of 0.1120 M Acetic acid titrated with 0.4750 M KOH. Calculate the initial pH, and the pH at the equivalence point of titration? Acetic Acid Dissociation Constant: 1.75 x 10 -5 ​
• A solution of weak base has pH = 7.95. What are the concentrations of the weak base and its conjugate acid ion in this solution? Ka = 6.28*10(-5). BOH <-------> B(+) + OH(-)
• Question #00257
• Question #4eab6
• Question #8dd75
• Question #11dcb
• Question #a8da2
• Question #99405
• Question #68f3f
• Question #d408a
• Question #d40e3
• Question #d9358
• Question #3478a
• Question #e7519
• Question #1bb81
• Question #eed26
• Question #f0437
• Question #14369
• Question #71432
• Question #cda49
• Question #87990
• Question #dadfd
• Question #66b60
• Question #bd6c1
• Question #5c07c
• Question #a3dd1
• Question #2b095
• How do you solve for Ka when you only have molarity of the acid and pH?
• Question #823c6
• Question #0984e
• Question #50ffd
• Question #3808b
• Question #e67f8
• Question #c83dc
• If #15.0mL# of glacial acetic acid (pure #HC_2H_3O_2#) is diluted to #1.50L# with water, what is the pH of the resulting solution? The density of glacial acetic acid is #"1.05 g/mL"#
• Assuming equal concentrations, which of these salt solutions should have the highest pH? (Choices in answer).
• Question #aa498
• What happens to the pH of water as the temperature is raised ?
• Question #fdd69
• Question #c3719
• What is the #"pH"# of a #"0.20-M"# solution of formic acid?
• Question #753db
• Question #b0cc2
• Question #07316
• Question #0760a
• Question #62820
• What is #pH#?
• Question #13933
• Question #f4442
• Determine the [OH-] of a solution that is 0.100 M in F-? Determine the pH of this solution?
• Question #5e0ee
• Question #62d6f
• Question #cb24c
• Solve an equilibrium problem (using an ICE table) to calculate the pH of of each solution: a solution that is 0.18M of HCHO2 in 0.14M of NaCHO2. What is the pH?
• How would you calculate the pH of a substance after a titration of 10.19mL 0.10M HCl with 10.99mL 0.093M NaOH?
• Question #62737
• Question #a4ab2
• What would you predict if you had first mixed the catalase (100%) in semi solutions of varying pHs of 3, 5, 7, 9, 11? What would you predict would be optimum pH?
• Question #f0076
• Question #70830
• How is pH related to a solution's acidity?
• What is the pH of a solution that has a hydronium ion concentration of #1.00*10^-10# M?
• Consider a solution of a weak acid at a pH equal to its pKa. By how much would the pH change, and in which direction, if we added to this solution enough base to neutralize 10% of the total acid?
• Question #e8a1b
• What is the pH of a solution that is neither acidic nor basic?
• What is the pH of an aqueous solution of 0.364 M ethylamine (a weak base with the formula #C_2H_5NH_2#)?
• Are egg-whites acidic?
• Why should distilled water be boiled and cooled when determining its pH?
• What is the pH range for acids? For bases?
• Question #55acc
• A patient's urine sample gave a pH reading of 8.2. What is the value of #[H_3O^+]# in this?
• Question #dd490
• Question #55869
• If the pH of an aqueous solution of #"0.15 M"# #"HF"# is #2#, what is the percent ionization of #"HF"#?
• If #[H_3O^+] = 1.005 * 10^-5# M, what is the pH?
• The [OH-] of an aqueous solution is #4.62 * 10^-4# M. What is the pH of this solution?
• Question #a3b8b
• What is the pH of #2.34 * 10^-5# #NaOH# solution?
• Why is water neutral in pH despite the fact that it produces hydrogen and hydroxide ions?
• What is the pH of #1.2 * 10^-3# HBr solution?
• What is the pH and pOH if the H+ concentration is #1*10^-4#?
• What can you say about the proportion of hydrogen ions and hydroxide ions in a solution that has a pH of 2?
• What is the pH of a 0.01 M solution of the strong acid #HNO_3# in water?
• If 1 mmole of NaOH is added into a solution in which there is 8 mmoles of aspartic acid with a net -1 charge and 10 moles of aspartic acid with a ned -2 charge, what would the pH of the solution be?
• What is the pH of a #1.4 * 10^-2 M# NaOH solution?
• Calculate pH for 0.10 mole NH3 dissolved in 2L of 0.050 M NH4NO3?
• 0.10 moles of sodium cyanate dissolved in 250cm^3 distilled water ,calculate pH?
• In the titration of sulfuric acid with potassium hydroxide, how the potassium and sulfate ions affect the #pH# of the solution?
• Calculate pH for a solution prepared by mixing 25ml of 0.1 M HCl with 25ml of 0.2 M NH3.What is the color of the solution if three drops of phenolphthalein is added to the solution?
• What is the pH of a .001 M solution of HCl?
• Calculate the #"pH"# of #10^-8# #"M"# #"HCl"#?
• How should the autoprotolysis reaction of water evolve at HIGHER temperature than #298*K#?
• What is the logarithmic concentration of the hydroxide ion in aqueous solution?
• Question #afe36
• Question #135b1
• Calculate #pH# of #10^-9# #M# #NaOH#?
• If chemical substance has a pH balance of more than 7 what is it considered?
• Question #7aa1b
• Question #27fca
• If the pH of a solution is 7.6, what is the pOH?
• Question #1108e
• How can you correct the pH of a pool with a reading of 3?
• If the pH of a sample was 3, how many times more acidic is it than a sample with a pH of 6?
• The pH of lemon juice at 298 K is found to be 2.32. What is the concentration of #H_3O^+# ions in the solution?
• What is the #"pH"# of a solution of magnesium hydroxide given that #K_(sp) = 1.8 * 10^(-11)# ?
• Question #fcf52
• Question #2506e
• Question #cf57c
• Question #d417a
• Consider the titration of #100# #ml# of #0.1# #M# #HCl# with #0.1# #M# #NaOH#. Calculate the #pH# of the solution at the following stages: ?
• Question #c1d7c
• Given equal concentrations of sodium chloride and sugar in water, how would the osmotic pressure of the sugar solution compare to that of the salt solution....?
• Question #07916
• For a solution containing initial concentrations of #"0.0500 M"# #"HNO"_2# and #"0.0100 M HClO"#, what is the #"pH"#?
• The pH of a solution is 5.6. What are the hydrogen and hydroxide concentrations?
• How do you calculate the pH & pOH of a solution which has a hydroxide concentration of 0.0053 M?
• How do you determine the pH of a solution that has a hydroxide concentration of #9.3*10^-16# M? Is this solution acidic or basic?
• How do you calculate the pH of a 0.050 M sodium cyanide solution?
• What would the concentration of hydroxide anions be in an aqueous solution that has #["H"_3"O"^(+)] = "0.325 M"# ? Given: #K_w = 10^(-14)# #"mol"^2"L"^2#
• Question #5d860
• Question #46084
• Question #2bd63
• Question #0209f
• Question #7db12
• What is the pH of a #4*10^-2# #M# #HCl# solution?
• Question #85a11
• Question #92c8a
• If #pH=0.325# for an aqueous solution, what is #[HO^-]#?
• Question #d5593
• What is the pH of a solution with #[OH^-] = 1*10^-4# #M#?
• What is the #[H_3O^+]# in a solution with #[OH^-] = 2.3 * 10^-12# #M#?
• What is the pOH of 2.15 M #Ba(OH)_2# solution? Is the solution neutral, acidic, or basic?
• What is the pH of a #6.49 * 10^-3# #M# #KOH# solution?
• What is the pH of a 0.0605 M solution of sodium hydroxide, #NaOH#?
• What is the pH of a 0.1 M acid solution?
• Question #1f9af
• What is the H+ concentration (in molarity) of a solution with a pOH of 6.7?
• An aqueous solution has a hydronium ion concentration of #6 * 10^-9# mole per liter at 25°C. What is its pH?
• A certain solution has pH 3.89 at 0°C. What is the pOH and #[OH^-]#?
• What is the pH of a solution with a hydrogen ion concentration of #3.5*10^-4#?
• Question #bdf57
• What is the pH of a solution that contains #7.8 * 10^-6# #M# #OH^-# at 25°C?
• What is the #[H^+]# in a solution that has a pH of 3.35?
• Question #fdeda
• Question #2c065
• Question #fe332
• What is the hydrogen ion concentration of a solution with pH = 3.75?
• What is the pH of a 0.0235 M #HCl# solution?
• Question #ab4a2
• Hydrofluoric acid, HF, has an acid dissociation constant of #6.8 * 10^(-4)# at 25 °C. At equilibrium the concentration of HF is 0.025M. a. What is the equilibrium constant expression for this dissociation? b. What is the pH of this solution?
• What is the pH and pOH of a #1.5 * 10^-3# M solution of sulfuric acid (#H_2SO_4#)?
• How do you convert pH to pOH?
• What is the pH of a 0.01 M solution of the strong acid #HClO_4#, perchloric acid?
• A solution of an acid in water has a pH of 4, which is slightly acidic. Is this solution a weak acid?
• What is the pH of a 0.35 M #NH_4Cl# solution?
• What is the pH of a 0.85 M #NH_4Cl# solution?
• Question #c3d97
• What is the pH of a .500 M solution of #HNO_3#?
• What is the pH of a #6.2 * 10^-3# M solution of #HF#?
• What is the #[H^+]# of a solution with a pH of 6.6?
• Question #4e291
• Is sparkling water acidic?
• What is the pH of #1 * 10^-4# #M# #NaOH#?
• Question #9190f
• A #10^-3 M# solution has been diluted to 100 times.Calculate the pH of the diluted solution?
• What is the pH of a 0.000460 M solution of #Ca(OH)_2#?
• Trimethylamine, (CH3)3N, is a weak base (Kb = 6.4 × 10–5) that hydrolyzes by the following equilibrium: (CH3)3N + H2O → (CH3)3NH+ + OH– What is the pH of a 0.1 M solution of (CH3)3NH+? (Enter pH to 2 decimal places; hundredth's.
• What is the pH of a 0.0067 M KOH solution?
• What is the pH of a #1*10^-4#M #HCl# solution?
• An #HCl# solution has a concentration of #3.26 * 10^-2# #M#. What is the pH of this solution?
• A solution of #NaOH# has a concentration of #5.51*10^-3# #M#. What is the pH of this solution?
• Question #e901d
• What is the pH of a 0.050 M NaOH solution?
• What is the pH at the equivalence point when 35.0 mL of 0.20 M ammonia is titrated by 0.12M hydrochloric acid? #K_b# for ammonia is #1.8 xx 10^(-5)#
• A solution has #[H^+] = 2.0 * 10^-5# #M#. How do you find the pOH of this solution?
• What is the ph of 0.45 M of #H_2SO_4#?
• The pH of a solution is 10. What is its #[H^+]# concentration?
• What is the pH of a .025 M #HCl# solution?
• The hydrogen ion concentration for a solution of #HBr# is #3.5*10^-11#. What is the pH for this solution?
• What is the pH of a solution that has an #OH^-# concentration of #1*10^-9# #M#?
• A 0.500M solution of a weak acid, HX, has a ka=3.26x10^-5 a) What is the pH of this solution? b) What is the percent ionization? c) What would be the pH be in a solution containing the strong electrolyte, 0.2M AlX3
• What are the pH of acids and bases?
• How does acid affect pH?
• How does acid relate to pH?
• How do you calculate the pH of acetic acid?
• How do you calculate the pH of a weak acid?
• How do you lower your acidity pH?
• How do you determine the pH of citric acid?
• What is the pH acid rain?
• Why is body pH acidic?
• Why is low pH acidic?
• Why is lower pH more acidic?
• How can the pH of an acidic soil be adjusted?
• How can pH of acidic soil be raised?
• How can the pH of an acidic lake be increased?
• How can you raise the pH of acidic soil?
• How do pH values of acids and bases differ?
• How do you calculate the pH of an acid?
• How do you calculate the pH of a strong acid or base?
• How do you calculate the pH of acetic acid?
• How does acid affect the pH and H concentration when added to water?
• How does carbonic acid affect pH?
• How does pH affect amino acid charge?
• How does pH affect amino acid structure?
• How does pH change when a strong acid is titrated with a strong alkali?
• How does pH relate to acid concentration?
• How does the pH of acid change when a base is added?
• How does the pH of acid change when a carbonate is added?
• How does the pH of an acid change when an alkali is added to it?
• How does the pH of an acid change with dilution?
• How does the strength of an acid relate to pH?
• How do you calculate the pH of an acid base mixture?
• How do you calculate the pH of acid rain?
• How do you lower pH with muriatic acid?
• How does salt affect pH?
• What is is the pH of salt?
• What is pH of a salt solution?
• What pH do salts have?
• How do you find the pH of a salt?
• How does pH affect saltwater fish?
• How does salt affect the pH of water?
• How does salt change the pH of water?
• What is the pH of salt and vinegar?
• What is the pH of a salt and water solution?
• What is the pH of saltine crackers?
• What should the pH of salt water be?
• What is the pH of a solution that has a hydronium ion concentration of 0.050 M?
• Given the following information and assuming the final solution will be diluted to 1.00L, how much more HCl should you add to achieve the desired pH?
• What does a solution with higher pH level indicate?
• What is the pH of a #3.9*10^-8# #M# #NaOH# solution?
• The pH of a solution is 8.7, what is the pOH?
• If #Ca(OH)_2(aq)=0.01*mol*L^-1#, what is #pH# of the solution?
• Question #ddd5c
• Question #5a458
• What is difference between a pH of 8 and a pH of 12 in terms of H+ concentration?
• How many times more basic is a pH of 12 compared to a pH of 8?
• What is the pH of a solution with a concentration of #2.4*10^-5# molar #H_3O^+#?
• Question #f26bd
• If a 6.03 x 10-6.0 M solution of a weak acid is 20 % ionized, what is the pKa for the acid?
• Question #96b5e
• What is the hydrogen ion concentration in a urine specimen that registers a pH of 4 on a strip of pH paper?
• Question #873de
• Question #bcaa2
• What is the pH of an aqueous solution if the #[H^+]=0.055# #M#?
• A lake has a low pH. Is it acidic or basic? Would fish be healthy in this lake?
• What is the pH of a solution of #10^(-8)# M sodium hydroxide ?
• What is #pH# for a solution whose #[H_3O^+]=6.7xx10^-5*mol*L^-1#?
• Question #07d32
• If #HO^-=2.7xx10^-11*mol*L^-1#, what is #pOH# of this solution?
• Question #a35c1
• Question #ba1d8
• What is the relationship between the pH of water, vinegar, and ammonia?
• Question #7f247
• Which of the following has the greatest concentration of hydrogen ions? How is this determined?
• (1). Find the concentration of the weak acid HA given that #K_a=10^(-5)# and pOH = 11 (2). What is the concentration of #OH^-# in this solution?
• How to calculate the pH value of 0.0001 M #"HCl"# ?
• Question #ae736
• A solution is 1.0 M in acetic acid. Pure water is added to double the volume of the solution. ?
• Question #6a0a7
• What is the #pH# for a #0.020*mol*L^-1# solution of #HCl(aq)#?
• 100.0 mL of a pH=2.600 solution of hydrochloric acid is diluted with pure water to a new volume of 200.0 mL. Calculate the pH of the new solution?
• Consider a #"0.075 M"# solution of ethylamine (#"C"_2"H"_5"NH"_2#, #K_b = 6.4xx10^(-4)#). Calculate the hydroxide ion concentration of this solution, and calculate the pH?
• What is the pH of a #"10 mL"#, #"0.10 M NH"_3# solution after the a) addition of #"0.10 mL 1.00 M HCl"# b) of another #"0.10 mL 1.00 M HCl"# c) addition of #"0.10 mL 0.10 M NaOH"# and d) addition of another #"0.10 mL 0.10 M NaOH"#?
• Calculate the pH of the solution below. 30.00mL of 0.100 M #"HCl"# is mixed with 25.00 mL of 0.100 M #"NH"_3# ?
• What is the pH after mixing the following?
• What is #pH# for a solution prepared from a #5.7*g# mass of sodium hydroxide that is dissolved in a #100*mL# volume of water?
• A solution of NaOH in water is:(i)golden yellow in colour (ii) pale green in colour (iii)sky blue in colour (IV)colourless (PLs experts and urgently with reasoning)?
• What is the pH of a 10 mL, 0.1 M NH3 solution when a 0.1 mL, 0.1 M NaOH solution was added into it?
• The # H_3O^+# concentration of a solution is equal to 0.8 M. What is the pH of the solution?
• What is #pH# of a #0.002*mol*L^-1# solution of #HCl(aq)#?
• What is the pH of a 0.05 M solution of sodium ethanoate ?
• Why does calcium hydroxide raise soil pH?
• Question #8eff7
• What is the pH of 0.35 M #KOBr# solution?
• Question #df7ec
• Question #12f80
• What is the #pH# of a mass of #4.66*mg# of barium hydroxide dissolved in a #1*L# volume of water?
• Which of the following solutions at equimolar solution would give the LOWEST #pH#?
• A #0.0729*g# mass of #HCl(g)# was dissolved in a #50*mL# volume of water. What is #pH# of this solution?
• What is the #pH# of an aqueous solution prepared from a #600*mg# mass of #NaOH# dissolved in #75*mL# of water?
• Question #197e4
• Question #b992c
• Question #44429
• Question #a20b5
• If a solution has pH 2.5 then is it acidic or alkaline and what are the concentrations of H+ and OH- ions?
• Question #a1253
• A total of 100. mL of 0.1000M HClO (Ka= 3.0x10-8)is titrated with 0.0100M KOH at 25C?
• How can human activities change the pH of the environment?
• How do chemical buffer systems resist changes in pH?
• What is pH when #[H^+] = 8.43 * 10^-4# #M#?
• A patient with respiratory alkalosis has a blood plasma pH of 7.58. What is the #[H_3O^+]# of the blood plasma?
• A solution with a pH of 10 is 100 times more basic than a solution with pH 8. Why?
• If you want to prepare a solution that has #"pH" = 8.51# at #25^@ "C"#, what initial concentration of #"NaF"# would you need to achieve?
• Question #3b25a
• What is the pH of a #1.0 x 10^-5# M solution of NaOH?
• What is the normal range for the pH of urine?
• Question #ab9ff
• The [#H^+#] in a solution is 0.01 M. What is the pH of the solution?
• What is the pOH of a solution with a pH of .7?
• Calculate the pH of a solution formed by the addition of 10.0mL of 0.050M hydrochloric acid to a 50.0mL sample of 0.20M acetic acid?
• What is the [OH-] concentration of NaOH solution with a pH of 9.4?
• What is the ph of a 100 ml solution containing 0.0040 g of HCl?
• Question #8a714
• Why do we use the pH scale to indicate the acidity of a solution rather than simply stating the concentration of hydronium ions?
• A #0.200*g# mass of sodium hydroxide is dissolved in a #0.500*L# volume of water? What are #pOH#, and #pH# of this solution?
• Question #5fd98
• Question #aca6e
• What are the units of base dissociation constant Kb ?
• What does pH measure?
• The pH of water is a measure of what?
• What is the pH or a solution with #[H^+] = 7.0 times 10^-7#?
• Question #7c41a
• How to calculate ph value of the solution? Two salt buffer.
• Question #31148
• Your tank of alkali fish needs a pH of 8, and the pH is 6 at present. What should you do to the #H^+# concentration?
• Question #e120d
• Why are #pH# and #pOH# defined on the logarithmic scale?
• Question #36e0b
• The pH of a solution changes fro 300 to 6.00. By what factor does the #[H_3O^+]# change?
• What are #pH# values for #1*mol*L^-1# solutions of #NH_4^+#, and #Na^+""^(-)OCl#?
• Question #ab631
• Question #984b3
• How do you determine the pH of a 0.125 M solution of nitric acid?
• Question #b36f6
• What would you expect the pH of an antacid to be?
• Question #f873f
• Question #5cf09
• What considerations apply when a weak acid is titrated with a strong base, as opposed to a strong acid with a strong base?
• What is the concentration of hydroxide ions in a solution that has a pH of 6.0?
• Question #f84ab
• In a #0.70 M# solution of benzoic acid, what percentage of the molecules are ionized (CHEMISTRY 1B problem)?
• Question #721ab
• In what range (0-7 or 7-14) would you expect the pH of KOH to be?
• What is the pH of a solution in which #1\times10^(-7)# moles of the strong acid, HCl is added to one liter of water?
• For a solution that is 0.285 M #HC_3H_5O_2# (propionic acid, #K_a=1.3×10−5#) and 0.0888 M HI, calculate the following?
• Calculate the pH and the concentrations of all species present, #"H"_3"O"^(+)#, #"F"^(-)#, #"HF"#, and #"OH"^(-)#, in #"0.05 M HF"# ?
• Question #0e9a3
• Question #ad47d
• Given the following, which pH indicator should the scientist use?
• What does the pH scale measure?
• What is the pH reading of stomach acid?
• What is the pH of #3.1 times 10^-3# #M# #HCl#?
• The pH of a soft drink is determined to be 4.0. What is the #[OH^-]# of the drink?
• What is the #[OH^-]# of a #4.0 times 10^-4# #M# solution of #Ca(OH_2)#?
• The pH of a fruit juice is 3.2. What is the hydrogen ion concentration of the juice?
• What will happen to the pH of a substance if the concentration of hydrogen #[H^+]# ions increases from #1.0 times 10^-8# to #1.0 times 10^-6#?
• Question #f372a
• What is the pH of a solution with #[OH^-] = 2.0 times 10^-10# #M#?
• The #[-OH]#] in a sample of egg whites is #6.3 times 10^-7# #M#. What is the #[H_3O^+]# in these egg whites?
• In neutral water under standard conditions, what are #[H_3O^+]#, and #[HO^-]#?
• What is #pH# and how is it defined?
• What is the pH of a 0.26 mol/L solution of methylamine (#"CH"_3"NH"_2, K_text(b) = 4.4 × 10^"-4"#)?
• What is the resultant #pH# of the solution.....?
• Calculate the #"pH"# for #"0.270 M"# benzoic acid? #K_a = 6.5 xx 10^(-5)#
• Is a solution with a pOH of 12.1 acidic, basic, or neither?
• When a weak acid, for which #K_a=6,2xx10^-5# is titrated with a strong base, what is the #pH# at half-equivalence?
• If #pH-=8.25#, what is #[H_3O^+]#?
• Which solution has a greater concentration of hydrogen ions (H), a solution with a pH of 3 or one with a pH of 7?
• As the pH number of an acid decreases, what happens to the strength of the acid?
• If the pH of Coca-Cola is 3.0 then it is considered to be what?
• What are 2 ways pH is relevant in your life?
• Why do indicators change colour at convenient points during a titration?
• Represent the autoprotolysis of water, and explain how #pH# defines the acidity of the solution. How are #pH# and #pOH# defined?
• What is the pH of a .20 M #NH_4NO_3# solution?
• What is the pH of a 0.027 M KOH solution?
• What is the pH of a 0.470 M solution of methylamine?
• Approximately what is the pH of a 0.1 M acetic acid solution?
• Question #1fb6d
• If the #K_b# of a weak base is #1.2 times 10^-6#, what is the pH of a 0.34 M solution of this base?
• When a bottle of wine is opened, its hydrogen ion concentration, #[H_3O^+]=4.1xx10^-4*mol*L^-1#; what is its #pH#? How does the #pH# evolve after the wine is left to stand?
• Question #0813e
• What do we mean by #H^+# or #H_3O^+# in acid-base chemistry?
• Question #18f54
• What is #pOH# of a solution prepared by adding a #15.8*mg# mass of potassium hydroxide to #11*mL# of solution?
• What is the #pH# of an aqueous solution in which #[HO^-]=0.041*mol*L^-1#?
• What is the pH of 2 M aluminium nitrate ?
• Question #881f7
• In a reaction of an acid with a base, the pH changes to a value that is closer to what?
• An unknown solution changed the color of a phenolphthalein indicator from coloriess to pink. What would you comment about the pH of the unknown solution?
• Question #1497e
• Question #d4fbe
• What is the pOH of a 0.001 M HCl solution?
• What are the hydronium and hydroxide ion concentrations in a solution that has a pH of 12.330?
• What does the pH of a fluid measure?
• Referring to the pH chart, how many times more acidic is a solution of pH 1 than a solution of pH 2?
• Why do solutions of barium chloride, and barium fluoride give rise to solutions with different #pH# values?
• Question #27dc1
• Why do fluoride salts give basic solutions in water?
• Question #82bc1
• How do you calculate the pH of 0.075M KOH?
• What is the pH of our drinking water?
• If #[H_3O^+]=4.5xx10^-3*mol*L^-1#, what are #pH#, and #pOH#, and #[HO^-]#?
• What number is considered neutral on the pH scale?
• How does the #pH# of an aqueous solution as #[H_3O^+]# is INCREASED?
• Question #76220
• The pOH of a solution is 2.0. What is its pH?
• Question #ca771
• Question #9d0d1
• What is the #[OH^-]# for a water solution if the #[H_3O^+]# is #6.0 times 10^-11# #M#?
• Question #418b5
• Given two aqueous solution whose respective #pH# values are #6# and #3#, how much more acidic is one solution compared to the other?
• Question #79114
• Question #8d00e
• A solution has a pOH of 6.39. What is the solutions pH? (You must answer to the correct number of s.d.'s)
• Question #42173
• A 0.01 M solution of an acid has a pH = 5.0. What is the Ka value?
• Of these, what is the order from highest pH to lowest pH? #LiOH(aq)#, #HBrO(aq)#, #Sr(OH)_2(aq)#, #NH_3(aq)#, and #HI(aq)#
• What does it mean when a substance has a pH greater than 7?
• The pH of a 2M solution of NaOH is...? (please include the complete solution of the problem)
• What is the concentration of hydronium ions in a solution at 25°C with a pH of 4.282?
• Question #fdc63
• What is the pH of 0.09 M solution of HBr (hydrobromic acid)?
• Question #29b74
• Which type of solution is one with a pH 8?
• The pH scale runs from a low of what?
• The pH of a solution is 7.0. What is the pOH?
• Question #9ff52
• If #"0.50 M"# of #"NH"_4"OH"# were to dissociate in water, and #K_b = 1.773 xx 10^(-5)#, what is the resultant #"pH"# at equilibrium?
• What is #pH# if #[H_3O^+]=0.001*mol*L^-1#?
• What is the concentration of hydrogen ions in a solution of pH = 4.0?
• When the pH of a solution is 12.83, what is [H+]?
• Question #8bf92
• What is the #K_a# for #"HNO"_2# if its starting concentration of #"0.14 M"# decreased to #"0.11 M"# by the time the reaction species reached equilibrium?
• What #["OH"^(-)]# and #"pOH"# give a basic solution?
• Question #0ce76
• Question #917b3
• Question #0059f
• What is #pH# if #(i)# #[H_3O^+]=5.6xx10^-5*mol*L^-1#; and #(ii)# if #[HO^-]=10^-7*mol*L^-1#?
• What is the #"pH"# of #"0.1 N"# #"Ca"("OH")_2#? Thanks.
• PH of #0.1(N)CH_3COOH# is what?
• What is #pH# of the solution if #a.# #41*mL# of #0.310*mol*L^-1# #NaOH(aq)# is added to if #31*mL# of #0.310*mol*L^-1# #HCl(aq)#? And #b.# if a #31*mL# volume of #0.310*mol*L^-1# of #HCl(aq)# solution are added to #21*mL# #0.410*mol*L^-1# #NaOH#?
• What should be the pH after 33 ml of 0.1 M NaOH was added to 40 ml of 0.05 M HCl?
• #60 ml# #0.2(N) H_2SO_4+40 ml# #0.4(N) HCl# is given. What is the pH of the solution?
• Question #f096c
• In terms of #pK_a#, which acid will be stronger? How does #pK_a# relate to #pK_b#?
• Question #6f85f
• What is the #pH# of a solution of #KBr#?
• What happens to pH if you dilute an acid?
• Question #00c91
• Question #c8443
• What is #[H^+]# if #pH=4.18#?
• What is #[HO^-]# in an aqueous solution for which #[H_3O^+]=3.2xx10^-3*mol*L^-1#?
• Question #d19cf
• Question #702e2
• Calculate the change in pH for a buffer solution with an initial pH of #3.9# after addition of #"0.1 M HCl"#?
• The Ka value of a weak acid, HA, is 10-6. An initial solution containing 1.0 M of HA is prepared. What is the pH of the final solution at equilibrium?
• pH of #0.1(M)# #NaH_2PO_4# is what?
• What is the #pH# of a solution of #"sulfuric acid"# of #2xx10^-2*mol*L^-1# concentration?
• What is the #"pH"# for an aqueous solution with #["H"^+] = 7.5 xx 10^(-3) "M"#?
• Question #ef8de
• What is the #"pOH"# of a solution containing #7.5 xx 10^(-2) "M H"^(+)#?
• What is the #"pH"# of a solution with #["OH"^(-)] = 3.9 xx 10^(-8) "M"#?
• How do you calculate the pH of 0.15 M aqueous solution of hydrazine?
• Question #b7542
• Question #32d3e
• What is the #pH# of a solution comprising #100*mL# volumes EACH of #HCl(aq)# at #0.20*mol*L^-1# and #NaOH(aq)# at #0.18*mol*L^-1#?
• How do we define #pH#?
• 1. If the pH of a solution is ….. the solution is basic. a. 2 b. 5 c. 7 d. 10 Can someone help me?
• Question #f777d
• Can pH levels go beyond 14?
• Question #dcad3
• How does #CO_2# cause ocean acidification?
• #30.0" cm"^3# sample of a #0.480" mol/L"# solution of potassium hydroxide was partially neutralized by the addition of #18.0" cm"^3# of a #0.350" mol/L"# solution of sulfuric acid. Calculate the pH of the solution formed?
• Question #0c050
• What is the pH of a solution in which #"25.0 mL"# of a #"0.100-M"# solution of #"NaOH"# has been added to #"100. mL"# of a #"0.100-M"# #"HCl"# solution?
• What concentration of formic acid will result in a solution with #"pH" = 1.90#? The value of #K_a# for formic acid is #1.8 * 10^(−4)#
• Question #47ca5
• Question #fcf5e
• What is the #"pH"# of a #3.5 * 10^-3# #"M"# #"HNO"_3# solution?
• Question #8d970
• Question #18150
• Question #b41c8
• What is the pH of a #"0.150-M"# #"NaOH"# solution?
• Question #98abc
• What is the #"pH"# for an aqueous solution with a hydroxide concentration of #5 xx 10^(-3) "M"# at #25^@ "C"#?
• Question #9988f
• Question #44d2f
• If I dissolve a Tums tablet #("1000 mg CaCO"_3)# in #"25 mL"# of water, how do I calculate the #"pH"# of the resultant suspension? When done experimentally, it was between #9# and #10#
• Question #f7407
• What is the molar concentration of H3O+ in a cola that has a pH of 3.120?
• What is the pH of a buffer system that contains 0.170 M hydrocyanic acid (HCN) and 0.140 M sodium cyanide (NaCN)?
• Chemistry question over acid and bases? I am not sure what I am doing wrong.
• Question #0f970
• Question #7f814
• What is the pH of 0.001 M NaOH(aq) at 298 K?
• You have a #"500-mL"# #"HCl"# solution having #"pH" = 3#. Determine the amount of #"NaOH"# solid #("M"_M = "40 g/mol")# that must be added so that the #"pH"# of the solution is changed to #10# ?
• How to determine the pH of the following mixture and the amount of salt formed?
• Question #8818a
• How to Calculate the pH of 0.180 g of potassium biphthalate (pKa = 5.4) in 50.0 mL of water?
• Question #38939
• Calculate the #"pH"# of a solution that resulted when #"40 mL"# of a #"0.1-M"# ammonia solution was diluted to #"60 mL"# ?
• Calculate the pH during a titration when 9.54 mL of a 0.15 M HCl solution has reacted with 22.88 mL of 0.14 M NaOH?
• What is the #"pH"# of a #"0.49-M"# #"NaClO"# solution?
• Calculate the #"pH"# of a solution when #"1 g"# of acetic acid and #"4 g"# of sodium hydroxide are dissolved in #"2 L"# of water?
• What is the pH of a 0.026 M Sr(OH)2 solution?
• #"20.0 mL"# of glacial acetic acid (pure #"CH"_3"COOH"#) is diluted to #"1.30 L"# with water. The density of glacial acetic acid is #"1.05 g/mL"#. What is the pH of the resulting solution?
• What is the pH of #10^(-2)# #"M HCl"# solution?
• The venom of biting ants contains formic acid, #"HCOOH"#. What is the #"pH"# of a #"0.0700-M"# solution of formic acid?
• What is the #"pH"# of a #"1.5-M"# solution of ammonia? The dissociation constant of ammonia at #25.0^@"C"# is #1.80 * 10^-5#.
• Three beakers each contain #"100 mL"# of acidic solution with a #"pH"# of #3.00#. The acids in the beakers are #"HCl"#, #"HNO"_2#, and #"HI"#. If #"50 mL"# of #"0.1 M NaOH"# is added to each beaker, which resulting solution will have the lowest #"pH"#?
• Calculate the pH of a 0.10 M #H_3PO_4# solution that is also 0.0005 M #(NH_4)_3PO_4#?