Titration Calculations

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Questions

• How do you do acid base titration calculations?
• How do you use titration calculations to find pH?
• What is a redox titration and what is it used for?
• Why is titration used when standardizing a solution?
• Is titration suitable for sodium nitrate?
• How can I do redox titration calculations?
• How can I calculate the titration of a weak acid and a strong base?
• How can I make back titration calculations?
• How does titration affect molarity?
• How does the endpoint of a titration differ from the equivalence point?
• How does pH change during titration?
• How does pKa affect a titration curve?
• How does CO2 affect titration?
• How does a back titration differ from a regular titration?
• How do you calculate the endpoint of a titration?
• How do titration curves work?
• How can titration be used to determine concentration?
• How can titration be used for medical testing?
• What is the titration curve of glycine?
• What is a titration curve?
• What is an example of a titration practice problem?
• What are some examples of titration?
• What is titration?
• Question #21700
• Question #c47f5
• If #"25 cm"^3# of a solution of calcium hydroxide with a concentration of #"1 g/dm"^3# takes a titre of 25 cm^3 of hydrochloric acid, what is the molar concentration of the #"HCl"#?
• Question #71ce2
• Question #05707
• Question #93f99
• Question #227e7
• Question #888f9
• Determine the initial pH, the pH at the midpoint (halfway to the equivalence point), and the pH at the equivalence point if 25.00mL of 0.1335 M NH3 (NH4OH) is titrated with 0.2350M HCl? Kb = 1.75*10(-5)
• Question #ff6ba
• Question #536b8
• 0.100M NaOH is used to titrate 50.0 mL of 0.100M HCl. Calculate the pH at 4 different points in the titration? a.) Initial pH of acid b.) After 40.00 mL of NaOH is added c.) After 50.00 mL of NaOH is added d.) After 50.20 mL of NaOH has been added
• A student prepares a solution of hydrochloric acid that is approximately 0.1 M and wanted to determine its precise concentration. A 25.00 mL portion of the HCl solution is transferred to a flask, and after a few drops of indicator are added, the HCl ?
• Question #010a5
• Question #4d7c4
• Question #b7836
• Question #f131c
• Question #20332
• Question #0c20b
• Question #c6e65
• Question #bab14
• Question #b0e61
• What volume in milliliters of #9.950*10^(−2)"M"# sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 17.0mL sample of 0.114M phosphoric acid?
• 3.6 #g# of oxalic acid (#H_2C_2O_4 * 2H_2O#) are dissolved and the volume is made upto 150 #ml#. Calculate the normality of the solution for redox titration?
• Question #a225d
• Question #db107
• Question #760bf
• An equimolar mixture of a weak acid and a strong base has a pH > 7 at the equivalence point. Which of the following describes the reaction that occurs at that equivalence point?
• Question #239b8
• Question #740df
• Question #e32b6
• Question #41c9a
• In an acid-base titration, would temperature conditions be a source of systematic error?
• What is the purpose of titration?
• A 30 ml volume of HCl is titrated with 23 mL of 0.20 M NaOH. How would you calculate the molarity of HCl in this solution?
• What is titration used for?
• What is a titration reaction?
• What is the function of an indicator in a titration?
• How does the process of titration work?
• What is the general equation for an acid base titration?
• If you titrate nitric acid with sodium hydroxide, you will add a drop or two of phenolphthalein to the sample of acid before you begin adding the sodium hydroxide. Why is the indicator added?
• What is the pH when 25.00 mL of 0.20 M CH3COOH has been titrated with 40.00 mL of 0.10 M NaOH?
• What is the pH of (CH3)3N solution, in a titration of 25mL of 0.12M (CH3)3N with 0.1M HCl, and Kb = 6.3 x 10^-5?
• What is the pH at the equivalence point when 35.0 mL of 0.20 M ammonia is titrated by 0.12M hydrochloric acid? Kb for ammonia is 1.8 x 10-5.
• How is a back titration lab carried out?
• In a titration, 16.02 mL of 0.100M NaOH was required to titrate 0.2011 g of an unknown acid, HX. What is the molar mass of the acid?
• Why do you use phenolphthalein as an indicator in titration of KHP and NaOH?
• Question #5c9d3
• Question #71616
• Question #38499
• A #40.16*mL# volume of sodium hydroxide solution with concentration of #0.1693*g*mol^-1# reached an endpoint with a quantity of oxalic acid. If the oxalic acid was initially dissolved in a #30.00*mL# what was the concentration of oxalic acid?
• Question #05209
• How do we quantitatively represent the oxidation of sodium thiosulfate, #S_2O_3^(2-)#, by dichromate ion, #Cr_2O_7^(2-)#?
• Question #0769b
• Question #7f583
• Question #7f640
• Question #989c7
• Question #b4f98
• Question #bd15c
• What do we mean by #"back titration"#?
• How do we represent the oxidation of oxalate ion by permanganate ion?
• Question #a0330
• Question #13d4e
• Question #d09d7
• What are equivalnts and milliequivalents?
• Question #636b5
• The titration of an impure sample of KHP found that 36.0 mL 0.100 M NaOH was required to react completely with 0.765 g of sample. What is the percentage of KHP in this sample?
• The titration of 20.0 mL of an unknown concentration #H_2SO_4# solution requires 83.6 mL of 0.12 M #LiOH# solution. What is the concentration of the #H_2SO_4# solution (in M)?
• Question #9b388
• In a titration experiment, 12.5 mL of 0.500 M #H_2SO_4# neutralizes 50.0 mL of #NaOH#. What is the concentration of the #NaOH# solution?
• A 35.0 mL sample of 0.225 M #HBr# was titrated with 42.3 mL of #KOH#. What is the concentration of the #KOH#?
• Question #1b658
• How much perchloric acid will react with a #20*mL# volume of sodium hydroxide whose concentration is #0.060*mol*L^-1#?
• Question #c81fe
• Question #c882e
• What volume must the final solution reach if you want to make a #"0.01 N"# oxalic acid solution in water using #"126 g"# of oxalic acid solid?
• In a certain titration, 34.5 mL of 0.20 M #NaOH# is required to neutralize 15.3 mL of #HCl#. What is the concentration of the acid (in normality and molarity)?
• What is the molar concentration of hydrogen ions if 12 drops of a benzoic acid #HC_7H_5O_2# solution are titrated with 26 drops of a .40 M #KOH# solution?
• What is the formula for solving titration problems?
• What requirements must be passed for a reaction to be feasible for titration?
• Why are titration problems done with vigorous swirling?
• Consider the titration of #50.0 mL# of #0.20 M# #NH_3# Kb #1.8x10^-5# with #0.20 M# #HNO_3#. How do you calculate the pH after addition of 50.0mL of the titrant?
• Using the correct amount of significant figures, how many milliliters of 8.48×10^(−2) M Ba(OH)2 (aq) are required to titrate 54.90 mL of 5.38×10^(−2) M H(NO)3?
• How do you calculate the molarity of the #HNO_3# solution?
• A 0.3240g sample of impure #Na_2CO_3# was dissolved in 50.00mL of 0.1280M #HCl#. The excess acid then requires 30.10mL of 0.1220M #NaOH# for complete neutralization. How do you calculate the % #Na_2CO_3# (MM = 105.99) in the sample?
• A 35.00 mL solution of 0.2500 M #HF# is titrated with a standardized 0.1532 M solution of #NaOH# at 25 degrees C. What is the pH of the #HF# solution before titrant is added? For #HF#, the Ka = 6.8 x 10–4 . W
• Consider the titration of 50 mL of 0.0200 M HCLO(aq) with 0.100 M NaOH (aq). What is the formula of the main species in the solution after the addition of 10.0 mL of base?
• How do you calculate the pH at the equivalence point for the titration of .190M methylamine with .190M HCl? The Kb of methylamine is 5.0x10^-4.
• How do you solve titration problems?
• What is the molarity of the potassium permanganate solution?
• How do you find volume in a titration question?
• How do you do titration problems involving pH?
• How do you solve titration problems?
• How do you do redox titration problems?
• How do you perform titration problems to find concentration?
• How do you do titration problems to find molarity?
• How do you solve titration problems for concentration?
• How do you solve titration problems for pH?
• How do you solve titration problems step by step?
• A 100.0 mL sample of 0.10 M #NH_3# is titrated with 0.10 M #HNO_3#. How do you determine the pH of the solution after the addition of 40.0 mL of #HNO_3#?. The Kb of NH3 is 1.8 × 10-5.?
• A 10.0 mL sample of #H_2SO_4# solution from an automobile battery requires 32.75 mL of M NaOH for a complete reaction. What is the molarity of the #H_2SO_4# solution?
• How many moles of HX have been added at the equivalence point?
• What is #"EDTA"#?
• Why is it necessary to standardize solutions of #"EDTA"# in complexometric titrations?
• Question #0bff5
• 29.4mL of an #CH_3COOH# solution were titrated with 18.5mL of a 0.175M #LiOH# solution to reach the equivalence point What is the molarity of the #CH_3COOH# solution?
• 50.0mL of an #H_2SO_3# solution were titrated with 36.90mL of a 0.100M #LiOH# solution to reach the equivalence point What is the molarity of the #H_2SO_3# solution?
• Given that it requires 31.0 mL of 0.280 M #Na_2S_2O_3(aq)# to titrate a 10.0-mL sample of #I_3^- (aq)#, how would you calculate the molarity of #I_3^- (aq)# in the solution?
• Consider the titration of 300.0 mL of #0.300 MNH_3 (K_b = 1.8 xx 10^-5)# with #0.300 M HNO_3#. What is the pH at the equivalence point?
• Why is #pH# important in a complexometric titration?
• Question #5a5e8
• Question #724b9
• Question #c8cd9
• A 25.0 mL sample of 0.105 M #HCl# was titrated with 315 mL of #NaOH#. What is the concentration of the #NaOH#?
• How does calcium hydroxide react with nitric acid?
• Question #bd69c
• A #31.27*mL# volume of sodium hydroxide at #0.167*mol*L^-1# concentration was used to neutralize a #22.5*mL# volume of AQUEOUS #H_3PO_4#. What is #[H_3PO_4](aq)#?
• Question #9ef0b
• If solution contains 0.85 mol of OH, how many moles of H+ would be required to reach the equivalence point in a titration?
• Question #0ae0f
• How to calculate the concentration of the acid solutions?
• Question #41ff8
• What volume of #0.5*mol*L^-1# #"sulfuric acid"# is required for equivalence with a #20*mL# volume of #0.5*mol*L^-1# #NaOH(aq)#?
• Does it matter if you spray a bit of water at the tip of your burette when titrating strong base into strong acid, i.e. does it change the equivalence point?
• Question #c434b
• Question #98e37
• A #21.8*mL# volume of #"potassium permanganate"# whose concentration was #1.68*mol*L^-1# achieved a stoichiometric endpoint when a volume of #100*mL# #H_2O_2(aq)# solution was added. What are #[H_2O_2]#, and the mass of hydrogen peroxide used?
• Why is it difficult to get the end-point of a titration with hydrochloric acid and sodium hydroxide when only a single titration is carried out?
• How does nitric acid behave in a titration?
• Strong base weak acid titration?
• What is #[HCl]# if a #25*mL# volume of #[NaOH]# of #0.250*mol*L^-1# concentration reaches an endpoint with a #22.5*mL# volume of the acid?
• If I don't know the concentration of the #"HCl"# that I am titrating with #"NaOH"#, can I still use the #"NaOH"# to titrate an unknown acid and determine its molar mass?
• Question #8fc4f
• Question #21460
• Question #8ed71
• What's V2 in general/how do you calculate it step by step?
• What is the theoretical point when the number of moles of added is equal to the number of moles of titrated in an initial solution?
• What was the percent by mass of aspirin in the tablets?
• Question #fa01b
• Question #bdb47
• The titration of 25 mL of a water sample required 15.75 mL of 0.0125 M EDTA. How do you calculate the hardness of water in the unit of ppm #MgCO_3#? (Assume the moles of EDTA are equal to the moles of MgCO3)
• Question #325c7
• Titration of an unknown amount of ascorbic acid, #C_6H_8O_6#, requires 25.4 mL of 0.100 M sodium hydroxide, #NaOH#. How do you calculate the grams of the ascorbic acid?
• Question #19c27
• A solution of 4.00 ml of #sf(Sn^(2+))# of unknown concentration is titrated against an acidified solution of 0.495M #sf(Cr_2O_7^(2-)#. The mean titre is 4.94 ml. What is the concentration of the #sf(Sn^(2+))# solution ?
• What is the technique you would use to separate and collect hydrated copper (ll) sulfate, #"CuSO"_4cdot5"H"_2"O"# from its aqueous solution?
• In a titration of 250.0 mL of methanoic acid (#"HCHO"_2#), takes 16.32 mL of 0.1004 mol/L NaOH to reach the end-point. What is the molar concentration of the methanoic acid?
• What should I know about a titration curve of strong base added into weak acid?
• Question #d77d9
• Question #18488
• If 26.23 mL of potassium permanganate solution is required to titrate 1.041 g of ferrous ammonium sulfate hexahydrate, #FeSO_4(NH_4)_2SO_4 * 6H_2O#, chow do you calculate the molarity of the #KMnO_4# solution.?
• Given the following, what is the molarity of the acetic acid? If the density of the vinegar is 1.006 g/cm what is the mass percent of acetic acid in the vinegar?
• How many mL #NaOH# will neutralize an acidic solution titrated with .0998 mol/L #NaOH#?
• How many mL of NaOH are needed to neutralize the acidity in a titrated solution containing .1234 g of #AlCl_3#?
• A 35.0mL sample of 0.150 M acetic is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added?
• At the endpoint of a titration of sodium acetate......will solution #pH# be at #7# or greater or lower than #7#?
• Question #84fcd
• What volume of #2.138*mol*L^-1# #NaOH# is required to react with a #25.0*mL# volume of #0.3057*mol*L^-1# solution of #"potassium pthalate"#, #1,2-C_6H_4(CO_2H)(CO_2^(-)K^(+))#?
• Question #a86ed
• Question #f8f90
• Is it possible for the equivalence point of a titration to not be at pH 7?
• How do you calculate the pH at the equivalence point for the titration of 0.140 M methylamine (#CH_3NH_2#) with 0.140 M #HCI#? The #K_b# of methylamine is #5.0x10^-4#?
• 10.00 mL of a weak base was titrated with 0.215 M HCl. When the titration is halfway to equivalence, 14.96 mL of HCl has been added and the pH is 10.18. What is the initial molarity of the weak base? What is the pH at equivalence?
• Question #fc90e
• A solution of sodium hydroxide is standardized against potassium hydrogen phthalate. From the following data, calculate the molarity of NaOH solution? (See details below)
• A 50.00 mL 1.5 M of #NaOH# titrated with 25.00 ml of #H_3PO_4# (aq). What is the concentration of the is #H_3PO_4# solution?
• Question #d5cf9
• Referring to the following information, if a 0.1593 gram sample of sodium carbonate, #Na_2CO_3# requires 31.45 mL of #HCl# solution for complete neutralization, what is the precise concentration of the acid?
• Will a precipitate form if 20 mL of #1 x 10^-7# M #AgNO_3# is mixed with 20 mL of #2 x 10^9# M #NaCl# at 25°C? For #AgCl#, #K_(sp) = 1.8 x 10^-10#
• Can a titration be applied to determine the concentration Na3PO4(aq) and NaH2PO4(aq) in a solution mixture of the two salts using HCl and phenolphthalein and methyl orange indicators?
• Can you help with this titration calculation ?
• How is #"Mohr's salt"# oxidized by #"potassium permanganate"# to give #Fe^(3+)# and #Mn^(2+)#? How is #"hydrogen peroxide"# oxidized by the same reagent to give #"dioxygen gas"#?
• Compute pH before/after addition of NaOH?
• The hexacyanoferrate(III) ion oxidizes Vitamin C (ascorbic acid, #"H"_2"Asc"#) to dehydroascorbic acid (#"Asc"#). What is the concentration of Vitamin C if 43.9 mL of #1.12 × 10^"-4"color(white)(l) "mol/L K"_3"Fe(CN)"_6# oxidizes 32.9 mL of Vitamin C?
• If #"0.35 g"# of #"KHP"# neutralized #"16 mL"# of #"NaOH"#, what is the #"NaOH"# concentration in molarity?
• Question #20f65
• Question #63681
• Question #3b9e4
• How many milliliters of 0.250 M KoH will be needed to titrate 12.53 mL of 0.130 M #HNO_3#?
• Question #6e960
• What volume of sodium hydroxide is required to titrate a #0.1*mol*L^-1# solution of acetic acid?
• What is #pH# when #HCl(aq)# is added to an aqueous solution of #"methylamine"#?
• 25 ml of a solution of barium hydroxide on titration with 0.1 molar solution of hydrochlroric acid gave a titre value of 35 ml . The molarity of sodium hydroxide is ?
• Question #765e0
• A #38.74*mL# volume of #0.50*mol*L^-1# sodium hydroxide solution reaches a stoichiometric endpoint with #19.37xx10^-3*mol# of sulfuric acid dissolve in #50.0*mL# of solution. What is the concentration with respect to #"sulfuric acid"#?
• Question #733bf
• What will be the final pH on mixing 50 ml of 0.01 M methanoic acid with 50 ml of 0.01 M sodium hydroxide ?
• Question #a034f
• You have a vinegar solution you believe to be 0.83 M. You are going to titrate 20.0mL of it with a NaOH solution that you know to be 0.519 M. At what volume of added NaOH solution would you expect to see the end point?
• Question #b3ad7
• When #HNO_2# is titrated with #NaOH# to the equivalence point is the pH of the resulting solution greater than, less than or equal to seven?
• In a titration of 0.35 M HCl and 0.35 M NaOH, how much NaOH should be added to 45.0 mL of HCl to completely neutralize the acid?
• If 82.5 mL of 0.723 M #H_2SO_4# titrates completely with 34.0 mL of #Al(OH)_3# solution, what is the molarity of the #Al(OH)_3# solution?
• Question #5dec3
• What mass of sodium hydroxide do I need to neutralize 500 mL of 1 mol/L pamoic acid?
• When adding base to a weak acid, does the concentration of #"HA"# have a net increase after the endpoint?
• Why is the point in the titration when neutralization occurs called the equivalence point?
• Question #6cce5
• Question #90d0d
• What volume of 1 M sulfuric acid is needed to titrate a 12 ml sample of 0.45 M NaOH?
• What is the molarity of a sample of sulfuric acid if 28.00 mL of 0.18 M NaOH was required to titrate 10 mL of the sulfuric acid?
• In a titration, when the number of moles of the hydrogen ions equals of the number hydroxide ions, what is said to have happened?
• Question #b9b56
• What reaction vessel is typically used in an acid-base titration?
• Question #098cc
• Question #7259d
• Question #a0e03
• Predict the expected pH at the endpoint of the titration of weak acid and a strong base? Maleic Acid and NaOH?
• What volume (in mL) of .158 M KOH solution is needed to titrate 20.0 mL of .0903 M H2SO4 to the equivalance point?
• You titrated a 25.00 mL solution of .0350 M oxalic acid with a freshly prepared solution of KMnO4. If it took 37.55 mL of this solution, what was the molarity of KMnO4?
• Why is oxalic acid often used as a standard in acid-base titrations?
• Question #00338
• A #20*g# mass of phosphoric acid dissolved in #250.0*mL# aqueous solution, reaches a stoichiometric end-point with WHAT volume of #NaOH(aq)# at #0.120*mol*L^-1# concentration?
• A #10*mL# volume of oxalic acid was titrated with a #34.40*mL# volume of #NaOH(aq)# whose concentration was #0.250*mol*L^-1#. What was the mass of oxalic acid present in the initial #10*mL# volume?
• Can any body tell me why NAOH cant considered as a primary standard? please provide an equation to the answers thanks
• How does permanganate ion oxidize oxalate dianion to give carbon dioxide, and #Mn^(2+)#? Given #0.1467*g# of #"sodium oxalate"#, what was the concentration with respect to #"permanganate"# if #28.85*mL# were required for equivalence?
• Calculate the pH after addition of (a) #"30.5 mL"# of #"0.100 M HCl"#, and (b) at the second equivalence point, if the first equivalence point is reached after #"25 mL"# of #"HCl"# is added?
• Titration problem?
• Why is calcium carbonate used as standard solution?
• Question #2750c
• A #15.62*mL# volume of monoprotic acid reached a stoichiometric endpoint with #16.49*mL# of sodium hydroxide whose concentration was #1.175*mol*L^-1#. What is the concentration of the acid?
• Question #e41ef
• Equal volumes of #"0.25 M"# #"HNO"_2# and #"0.25 M"# #"HNO"_3# are titrated separately with #"0.25 M"# #"KOH"#. Which would be the same for both titrations?
• Question #006d1
• Feasibility of titration of #"2.5 mmols HY"# (#"pK"_a = 7.00#) using #"0.1 mmol/mL"# #"NaOH"#?
• Question #ed2aa
• What is the pH at the half equivalence point when 50.0 mL of 0.200 M NaOH is titrated with 0.100 M HCl? The starting pH is 13.3.
• You used 1.01 g of solid and it required 15.00 ml of 1.00 M HCL to reach the endpoint. determine the no of moles of hcl in your titration?
• The #"pH"# at one-half the equivalence point in an acid-base titration was found to be #5.67#. What is the value of #K_a# for this unknown acid?
• What volume of 0.1292 M NaOH is needed to neutralize 25.00 mL of HCl of unknown concentration?
• A #"25.0-mL"# sample of #"0.150-mol L"^(-1)# acetic acid is titrated with a #"0.150-mol L"^(-1)# #"NaOH"# solution. What is the #"pH"# at the equivalence point?
• Titration problem?
• A 30.00 mL sample of 0.100 M #"HOI"# is titrated using 0.100 M #"NaOH"#, #K_a=2.3xx10^-11# for #"HOI"#?
• What is the pKa of buffer solution #HC_2H_3O_2# when HCl is added?