pH calculations

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Questions

• How do you determine ph of a solution?
• How do you determine pH at an equivalence point?
• How do you determine pH from molarity?
• What does alkalinity mean?
• What is a base?
• How do acid base indicators change color?
• What is a neutral pH?
• How does alkalinity affect pool water?
• Why is pH important in drinking water?
• How can I calculate the pH of a solution?
• Question #81531
• Question #b2684
• Question #43ded
• Question #c74c8
• A 0.20 mol/L solution of propionic acid has a pH of 2.79. What is the #"p"K_text(a)# of propionic acid?
• How do pH and pKa relate?
• A 100mL sample of 0.10 M NH3 has a Kb of 1.8*10^-5. What is the pH?
• Question #41ee5
• A solution is prepared by mixing 88.0 mL of 5.00 M HCl and 26.0 mL of 8.00 M HNO3. Water is then added until the final volume is 1.00 L. How would you calculate [H+], [OH -], and the pH for this solution? please explain?
• How would you use the Henderson-Hasselbalch equation to calculate the ratio of H2CO3 to HCO3- in blood having a pH of 7.40?
• Can the Henderson-Hasselbalch equation be used to estimate the pH values at the equivalence point?
• What is the Henderson-Hasselbach equation?
• How do you derive the Henderson-Hasselbalch equation?
• How would you use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.17 M in HCHO_2 and 0.10 M in NaCHO2?
• Question #db69c
• Question #2c8ae
• What is the pH of a solution if the #[H^+] = 3.45 * 10^-9 M?#
• Ionic product of water at #310# #K# is #2.7# x #10^-14#. What is the #pH# of neutral water at this temperature?
• 20.00 ml of 0.10 M sodium carbonate is placed in a flask with phenolphthalein and methyl orange indicators present. 0.10 M hydrochloric acid is placed in the burette and run in slowly. How do you do the following calculations ?
• Question #0c50c
• A certain sample of #"HClO"_2# has a concentration of #"0.125 M"#. Calculate the pH at equilibrium. Why can we not treat #"HClO"_2# as a strong acid, even though #K_a > 1#?
• How is the pH of a solution related to the #[H_3O^+]#?
• A 100.0 mL sample of .10 M #NH_# is titrated with .10 M #HNO_3#. What is the pH of the solution after the addition of 150.0 mL of #HNO_3#?
• What is the pH of a solution whose #H_3O^+# concentration is #1*10^-9#?
• What is the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25°C?
• Question #c8734
• Question #0c2a7
• Question #eddcd
• What is the pH of a #1.15 * 10^-12# M solution of #KOH#?
• What is the #pH# of a #6.0*mol*L^-1# solution of #NaOH(aq)#?
• Question #69fd6
• A solution has a #[OH^-]# of #1*10^-2#. What is the #pOH# of this solution?
• What is the pH of a #1.0 * 10^-3# #M# sodium hydroxide solution?
• The pOH of a solution is 10.75. What is the concentration of #OH^-# ions in the solution?
• What is the hydronium ion concentration of a solution that has a pH of 8.57?
• Given a solution with a pH of 2.8, what is the #H^+# of the solution?
• Question #7e83a
• What is the pH of a solution with a #[H_3O^+]# of #3.45*10^-6# #M#?
• What is the #"pH"# for #2.5 xx 10^(-6) "M"# #"HCl"#?
• Question #01170
• If the pH is 14.75, what is #[OH^-]#?
• What is #[NH_4^+]# in a solution that is 0.0200 M #NH_3# and .0100 M #KOH#?
• A swimming pool worker wants the pool's pH to be 7.2. She comes by to test the water and finds that the pH is 6.2. What should she do to correct this situation?
• What is the concentration of hydronium ions in a solution with a pH = 3.9?
• If an acid has an #[H^+]# of #1*10^-2#, what is its pH?
• What is the pH of a #6.7x10^-5#M #H^+# solution?
• What is the #pOH# of a #6.5*10^-12# #M# #OH^-# solution?
• What is the #pOH# of a #5.6*10^-5# #M# solution of cesium hydroxide?
• What is the pH of a #1*10^-5# #M# solution of sulfuric acid?
• What is the pH of a #8.7*10^-12# #M# solution?
• What is the #pOH# of a #2.1*10^-6# #M# solution?
• What is the pH of a #2.6*10^-9# #M# #H^+# solution?
• What is the pH of a solution with [H+]= #2.3 x 10^-6#?
• What is the pH of a solution prepared by mixing 50.0 mL of 0.30 M #HF# with 50.00 mL of 0.030 M #NaF#?
• What is the pH of a 0.10 M solution of barium hydroxide, #Ba(OH)_2#?
• What are the concentrations of #H_3O^+# and #OH^-# in oranges that have a pH of 3.7?
• What is the #[OH^-]# in a solution that has a #[H_3O]=1.0*10^-6# #M#?
• What is the acid concentration of a sample of acid rain with a pH of 4.20?
• What is the pH and pOH of 6.5 g of sodium hydroxide in 650 mL of water?
• A 50 mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M HCl. What is the initial pH?
• How do you use the Henderson-Hasselbalch to calculate the pH of a buffer solution that is .50 M in #NH_3# and . 20 M in #NH_4Cl#?
• The #K_sp# of #Al(OH)_3# is #2*10^-32#. At what pH will a 0.9 M #Al^(3+)# solution begin to show precipitation of #Al(OH)_3#?
• When an aqueous solution at room temperature is analyzed, the #[H^+]# is found to be #2.0*10^-3# #M#. What is the #[OH^-]#?
• What is the pH of a #7.5x10^-3 M3 #H^+# solution?
• What is the pH of a #8.4x10^-6 M# #H^+# solution?
• Acid rain is a serious environmental problem. A sample of rainwater collected in the Adiron- dack Mountains had an H+ concentration of .001 mol/L. What is the pH of this sample?
• You have two bases: one has a pH of 8 and the other has a pH of 10. 10 How much stronger is the pH of ten than the other one?
• Aweak acid HA, has a pKa of 5.0. If 1.0 mol of this acid and 0.1 mol of NaOH were dissolved in one liter of water, what would the final pH be?
• What is the difference in hydrogen ion concentration comparing solutions with a pH of 2 and pH of 4?
• A pH of 5 is how many more times acidic than a pH of 6?
• What is the H+ if the pH of a solution is 1.65?
• What is the weak base ionization constant (#K_b#) for #HS^-# equal to?
• What is the weak ionization constant (#K_a#) for #HCN# equal to?
• What is the weak ionization constant (#K_a#) for #HCNO# equal to?
• A map of eastern North America, showing the pH of rainfall in the various states, indicates that the pH of rain in New York State varies from 4.22 to 4.40. According to these figures, what is the most acidic rainfall in New York?
• What is the pH of a 1.00 x 10^-4 M solution of lithium hydroxide solution?
• What is the pH when 0.600 moles of potassium benzoate (#KC_7H_5O_2#) has been added to 1.50 of water?
• What is a gas that dissolves readily in water to produce a solution with a pH of about 11?
• What is the pH of a 0.500 M solution of acetylsalicylic acid, pK 3.52?
• Since pure water is neutral in pH, what does it contain?
• If an alcohol solution has a pH of 5, would it be a primary alcohol, a second alcohol, a tertiary alcohol, or a phenol?
• What does a pH scale measure?
• On the pH scale, which numbers indicate a basic solution? An acidic solution? Why?
• What is the pH of a .200 M solution of formic acid?
• What is water on the pH scale?
• What is pH of tap water?
• What is the pKa of acetic acid?
• Given 100.0 mL of a buffered solutions which is 0.30 M #HF# and 0.30 M #NaF# and the Ka of #HF# to be 7.2 x 10^4, how do you find the pH of this buffer?
• How much more acidic is a solution of pH 3 compared with a solution of pH 6?
• Soap is made from a strong base and oil. Do you think the pH of soap is 4 or 9?
• What is the pH of a mixture that contains 0.60 M # HCl# and 0.30 M #HNO_2#?
• What is the pOH of an aqueous solution at 25.0 #"^o#C that contains #3.98 x 10^-9# M hydronium ion?
• What is the ratio of the moles of conjugate base to the moles of acid if the pH is 5.29 and the pKa is 5.150?
• If #pH=7.5#, what is #pOH#, and what is #[HO^(-)]#?
• How do I find #pH# and #pOH# for solutions of aqueous hydrogen fluoride or sodium fluoride?
• Why would determining the ph of cranberry juice be challenging?
• What is the Ph number of acid?
• What is the pH of normal rainwater?
• What is the pH of pure water at 25.0 °C if the Kw at this temperature is #1.0 x 10-^14#?
• The [#H^+#] (#H^+# concentration) in a solution is #1 x 10^-8# M. What is the pH of the solution?
• How do you determine the pH of a solution that is 3.85% KOH by mass? Assume that the solution has density of 1.01 g/mL.
• The #Ka# of phosphoric acid, #H_3PO_4#, is #7.6 x 10^-3# at 25#"^o#C. For the reaction #H_3PO_4(aq) -> H_2PO_4(aq) + H^+(aq)# #DeltaH# = 14.2 kJ/mol. What is the Ka of #H_3PO_4# at 60#"^o#C?
• How many grams of #SrO# should be dissolved in sufficient water to make 2.00 L of a solution with a pH= 11.00?
• What does a solution with a hydronium ion concentration of# 10^-11# M have a pH of?
• Question #14d2b
• Calculate pOH of a .1540 M solution of phenol (C6H5OH) Ka=1.61x10^-10?
• What is the pH of normal rain?
• What is the concentration of hydronium ions in a solution that has a pH of -3? Why is such a solution impossible to prepare?
• Which of the following pH measurements is the weakest acid; a pH of 4, a pH of 6, or a pH of 8?
• Given a solution of nitric acid whose #pH=4#, what are #[H_3O^+]#, and #[NO_3^(-)]#?
• What is the pH of unpolluted rain water?
• How do you calculate the pH of a 0.26 M methylamine solution?
• How do we get #"pH"# from #"pOH"#?
• How do we work out #[H_3O^+]# from #pH#?
• When the pH of a solution decreases by 1, say from pH = 3 to pH = 2, by what factor does the hydronium ion concentration increase? Why?
• Ammonia (#NH_3#) is a weak base with a #K_b = 1.8 x 10^-5#. What is the balanced chemical equation for the reaction of ammonia with water. Using the I.C.E the method, calculate the pH and ionization of a 1.75 M #NH_3# solution in 2.50 M #NH_4Cl#?
• If the hydrogen ion concentration in a solution is #7.10 x 10^-5# mol/L, what is the pH?
• If the pH of a solution is 3.437, what is the hydrogen ion concentration in mol/L?
• If the #K_a# of a monoprotic weak acid is #3.4 x10^-6#, what is the pH of a 0.14 M solution of this acid?
• Question #d327a
• When dissolved in equal volumes of water, which of the solutions will have a higher pH?
• If #K_a=2.0xx10^-11# for #"hypoiodous acid"#, #HOI(aq)# what is #[H_3O^+]# for #[HOI(aq)]#, whose concentration is #0.23*mol*L^-1#?
• Given #K_a = 5.90 xx 10^(-2)# for #"0.530 M"# lactic acid, what is the #["H"^+]# at equilibrium?
• Calculate the #"pH"# of a #"0.32 M"# solution of acetic acid (#K_a = 1.8 xx 10^(-5)#) to three sig figs?
• What is the #"pH"# for a solution containing #"0.500 M"# of a weak triprotic acid whose first #K_a# is #5.78 xx 10^(-10)#? Assume only the first proton is significant. Report your answer to two significant figures.
• #K_b# for #"acetoaminophen"# is #4.1xx10^-4#. What is #[HO^-]# for a solution of #"acetoaminophen"# at #0.910*mol*L^-1# concentration?
• When a general base associates in water, with #K_b# #"<<"# #10^(-5)#, what is the algebraic expression for #x# as a function of #K_b# and the equilibrium concentration of the base?
• Question #b8408
• What is the #pH# of a solution whose concentration is #0.450*mol*L^-1# in ammonia; #K_b=1.80xx10^-5#?
• Question #f622c
• If #pH=8.19#, what is #[H_3O^+]#?
• What is #[HO^-]# of a solution for which #pH=3.10#?
• Assuming #"Ba"("OH")_2# dissociates completely, what is the #"pH"# of #"0.015 M"# #"Ba"("OH")_2# to three sig figs?
• What is #[HO^-]# of a solution that is #6.80xx10^-2*mol*L^-1# with respect to #HBr(aq)#?
• What mass of benzoic acid, #C_6H_5COOH#, would you dissolve in 400.0 mL of water to produce a solution with a pH = 2.95?
• Question #6bf82
• Question #83440
• Question #4d832
• Question #08525
• How to calculate the pH of a solution that is 0.02500M CO2..?
• Question #12725
• What is the #pH# of a #0.200*mol*L^-1# solution of #HF#, for which #K_a=6.3xx10^-4#?
• Question #31b0a
• A #0.45*g# mass of #HCl# is dissolved in water to give a #300*mL# volume of solution. What are #pOH#, and #[HO^-]# for this solution?
• What is the #pH# of the final solution...?
• What is [H3O+] for a 0.500 M solution of hydrochloric acid? Make sure you include the ionization equation.
• Calculate [OH-] ions in a 0.125 M solution of nitrous acid. Is this solution acidic or basic; how do you know? Make sure you include the ionization equation.
• What is #pH# of an aqueous solution for which #[NH_4^+]=1.0*mol*L^-1#?
• Question #166b1
• What is #pH# for a #1.95*g# mass of pure sulfuric acid added to enough water to give a final volume of #1*dm^3#?
• What is #[H_3O^+]# for a solution whose #pH-=2.85#?
• How to calculate the number of H+ and OH- ions in this question?
• How do you calculate #[OH^-]# in #[H_3O^+] = 2.1 times 10^-8# #M# at 25°C?
• Question #2ce53
• Question #b7b14
• Question #baf96
• If #[H_3O^+]-=10^(-10)*mol*L^-1#, what is #pH# of this solution?
• What is the #pH# of a #0.10*mol*L^-1# solution of ammonium ion....for which #pK_a=9.26#?
• Question #9ebcd
• If #25*cm^3# of #1.0*mol*L^-1# nitric acid are reacted with. #50*cm^3# #0.5*mol*L^-1# #NaOH# what is the #pH#?
• Concentrated sulfuric acid (98.12 g.mol-1) has a density of 1.5 g/cm3 and is 60 % H2SO4 per mass. The rest is water. How many H+ ions are there in a 45ml concentrated sulfuric acid solution?
• What is the pOH if the pH is 11.25?
• What is the [#OH^-#] in a solution of pH 3.00?
• Calculate the pH of a solution with a pOH of 5. Is this solution acidic or basic?
• Question #4a1f3
• Question #27b41
• What will be the pH of the solution that results from the addition of 20mL of 0.01M Ca(OH)2 to 30mL of 0.01M HCl?
• A #5*g# mass of sodium hydroxide is dissolved in a volume of water such that the final solution is #1*L#...what are the #pOH#, and #pH# of this solution, and what is the final concentration of #H_3O^+#?
• What is #pH# of an aqueous solution that is #0.016*mol*L^-1# with respect to #NaOH#?
• How do you calculate the molar concentration of OH in a 0.075 M solution of ethylamine?
• What is the concentration of a solution of #K_2CO_3# that has pH = 11.90?
• Question #3cab0
• Question #e285b
• What would be the pH of a 0.503 M solution of ammonia (NH3) at room temperature? The #K_b# of ammonia is #1.78 x 10^-5#
• Question #8dd3e
• Question #98213
• Question #11a0b
• Question #66439
• If #[H_3O^+]=5.0xx10^-3*mol*L^-1#, what is #pH# and what is #pOH# of this solution?
• What is the pH of a solution with #[H^+] = 7.0 times 10^-12 "M"?#
• What is the pH of a solution made by mixing 100.0 mL of 0.10 M #HNO_3#, 50.0 mL of 0.20 M #HCl# and 100.0 mL of water? Assume that the volumes are additive.
• If #[H_3O^+]=1.2xx10^-8*mol*L^-1#, what are #pH# and #pOH#?
• Question #ee5b2
• Question #19ceb
• #"Hydroxylamine"#, #HONH_2# is a weak Bronsted base with #K_b=10^-8#. What is #pH# for a #0.024*mol*L^-1# solution?
• What is the #H^+# concentration for an aqueous solution with pOH = 3.05 at 25°C?
• What is the #H^+# concentration for an aqueous solution with pOH of 4.31 at 25°C?
• Given #K_b=2.22xx10^-11# for nitrite ion, what is #pH# for a solution of #NaNO_2(aq)# that is #4.5xx10^-4*mol*L^-1# with respect to the salt?
• Question #8556c
• A certain aqueous solution contains #"0.27 mols"# of weak acid #"HA"#. If #"12.0 mL"# of #"3.10 M"# #"NaOH"# was added to it, resulting in a #"pH"# of #3.80#, what is the #"pK"_a# of the weak acid?
• What is the pH of a solution prepared by mixing 50.0 mL of 0.010 mol/L HCl(aq) and 50.0 mL of 0.010 mol/L Ca(OH)2(aq)? Assume the temperature is 25 degrees celcius.
• What is #pOH# for a solution that is #0.565*mol*L^-1# in #HClO_4(aq)#?
• What is the pH of a #5.00 x 10^-2# M aqueous solution of #Ba(OH)_2#?
• What is the pH of a 0.00162 M NaOH solution?
• How would you determine the pH of 0.10 M #NH_3# solution? #NH_3# is a weak base with a #K_b# equal to #1.8 x 10^-5#.
• What is the pOH of a solution with an [OH-] concentration of #9.2 x 10^-8# M?
• What is the pOH of a solution with an [OH-] concentration of #9.2 x 10^-11# M?
• When an acid is added to a basic solution, what happens to the pH of the solution?
• If #pH=7#, what are #[H_3O^+]#, and #[HO^-]#?
• Question #672a6
• Question #d798c
• Question #00d80
• Question #d523c
• What is the resultant #pOH# when a #5*mL# volume of #NaOH# of #0.165*mol*L^-1# concentration is diluted to a #450*mL# volume?
• Solution A has a pH of 3 and solution Z has a pH of 6. How many times greater is the hydronium ion concentration in solution A than the hydronium ion concentration in solution Z?
• Question #6b487
• Does a solution with the concentration of [OH-] = 4.3 x #10^-5# M have a pH of 5?
• Question #fb9c4
• How do you calculate the pH of an aqueous solution of 0.0726 M potassium sulfite?
• Question #52060
• If #pH=2# upon dilution what is #[HClO_4(aq)]#?
• What is the pH of a solution with a hydronium concentration of #8.6 times 10^-8# #M#?
• How do you find the pH of a solution whose #[H^+] = 3.44 times 10^-12?#?
• Question #17d18
• 1)Calculate the pH of a 0.1M solution of NaOH ,knowing that the volume of the solution is 300mL. 2)Calculate the pH of a 0.3M solution of HCl , knowing that the volume of the solution is 250mL (?)
• A solution contains #[OH^-] = 4.0 times 10^-5# #M#, what is the concentration of #[H_3O^+]#?
• Question #29a9b
• What is the concentration of a lithium hydroxide solution that has a pOH of (3.1x10^0)? (answer to 2 s.d. in mol/L)
• What is the pH of a 6.2 x 10-2 mol/L solution of nitric acid?
• The concentration of H+ ions in a solution is #1.0 xx 10^-12# M. What is the pH of the solution?
• If #pOH=10# for an aqueous solution, what is #pH#?
• If #[H_3O^+] = 8.26 times 10^-5# #M#, what is the pH of the solution?
• Question #add52
• How do you calculate the pH of a .40 solution of #Ba(OH)_2# when 25.0 mL is added to 250 mL of water?
• Question #d9c3a
• What is the #"pH"# for #"0.11 M"# #"HF"# dissociating in water at #25^@ "C"#? #K_a = 7.2 xx 10^(-4)#
• How do you calculate the pH of this solution: #[H^+] = 8.3 xx 10^(-10)# M?
• How do you find the value of #[OH^-]# for a solution with a pH of 8.00?
• What is #pH# of a solution #1.2xx10^-2*mol*L^-1# with respect to #KOH#?
• What is #pH# of a solution nominally composed of #1.5*mol*L^-1# ammonia? #pK_b# #"ammonia"=4.3xx10^-5#
• What is the pH of a solution with [H+] = #2.3 times 10^-3#?
• What is the pH of a solution that has a hydronium ion concentration of #1.00 times 10^-4 M#?
• What is #pH# of a solution prepared from a #313*mg# mass of barium hydroxide dissolved in a #1*L# volume of water...?
• Question #4b2ef
• Calculate amount of formic acid (ka=2*10-4) which shoud be dissolved in 10L of water to obtain a solution of pH=3.7?
• Question #b80b1
• What is the pH of a solution that is 0.50 M in sodium acetate and 0.75 M in acetic acid?
• If the hydroxide ion concentration is #3.5 × 10^"-5"color(white)(l)"mol/L"#, what are the pH and the hydrogen ion concentration?
• The pH of a lime is 1.90. What is the #[H_3O^+]#?
• What is the equilibrium concentration of #"OH"^(-)# in a #"0.120 M"# solution of #"Na"_2"CO"_3#?
• Question #231e7
• Question #f1da9
• What is #pH# in the following scenario?
• Question #ed4f1
• Question #bc8f1
• What is the #"pOH"# for a solution of #4.8 xx 10^(-10) "M"# #"H"^(+)#?
• What is the concentration of hydroxyl ions in a solution of pH #8# ?
• If the #"pH"# is #6.49# and the three values of #"pK"_a = 2.148, 7.199, 12.15# for phosphoric acid, what species dominates in solution?
• Help me please?? Thanks!
• Can I get some help please? I really appreciate that and thank you!
• What is the concentration of HCl if its pH is 3?
• Question #3dd5d
• If #pH=1.65#, what is #[H_3O^+]#?
• What does it mean if a solution has a pH of 6.0?
• What are substances with a pH below 7.0 considered?
• Does the presence of an acid in a water solution affect the pH of the solution?
• What is a substance with a pH of 4 called?
• At 25 °C, how many dissociated H+ ions are there in 341 mL of an aqueous solution whose pH is 11.39?
• The pH of a #5.95\times 10^-1# M solution of a weak base is 11.54. What is the #pK_b# for this base to two decimal places?
• What is the pH of beer in which the hydrogen ion concentration is #5.6 \times 10^ -7# M?
• Question #1fbd7
• Question #5f23b
• A chemist dissolves 0.01 mol of an acid (HCl) in enough water to make a 350 mL solution of acid. What is the pH of the acid solution?
• What is the pOH of a solution that has OH concentration equal to #1.36×10^-10" mol"*"dm"^(-3)# ?
• What is the pH of [H3O+]=1.0 M? How do I solve for it?
• Calculate the pH of a #"0.2 M"# solution of #"NaC"_2"H"_3"O"_2# given that the hydrolysis constant is #K_h = 5.6xx10^(-10)#?
• What is the pH if 50.0 mL of 0.100 M HCN is mixed with 50.0 mL of 0.100 M NaOH?
• What is the pH if 50.0 mL of 0.100 M HCN is mixed with 100.0 mL of 0.100 M NaOH?
• What is the pH when #"100.0 mL"# of #"0.100 M HCN"# is mixed with #"50.0 mL"# of #"0.100 M NaOH"#...?
• 50.0 mL of 0.100 M #"NH"_3# is titrated with 0.100 M #"HCl"#. What is the pH of the #"NH"_3#/#"HCl"# mixture after the addition of 25.0 mL of #"HCl"#?
• A solution of formic acid has a pH of 2.70, calculate the initial concentration of formic acid?