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A student titrated 10.00 mL of 0.10 M sodium acetate (CH3COONa) with HCℓ and de…

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Wize University Chemistry Textbook > Acids and Bases

Autoionization of Water (Kw)

5 Activities

Wize University Chemistry Textbook > Buffers and Titrations

Titration Problems

2 Activities

A student titrated 10.00 mL of 0.10 M sodium acetate (CH3COONa) with HCℓ and determined that 10.00 mL of HCℓ was needed to reach the equivalence point. At equivalence, what is the expected pH?

Ka of CH3COOH = 1.8×10-5
More Autoionization of Water (Kw) Questions:
Concentration
A solution of LiOH is made by mixing an unknown amount of LiOH with 1 L of water. The pOH is measured to be 3.65, what is the concentration of LiOH?
MW Li: 7 g/mol
MW O: 16 g/mol
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H3O+ concentration in diet cola than in milk?
Acids and Bases: Ka
The following occurs when HCl is placed in water:
HCl <----> H+ + Cl-
The Ka for this reaction is known to be Ka = 5.64 once it reaches equilibrium. At equilibrium, 1.35 x 10-7 M of HCl and 1.2 M of Cl- can be found. What is the pH of the solution at equilibrium?
Acids and Bases: pH
100 mL100\ mL of a 0.5 M0.5\ M solution of Hydrochloric acid (HCl\rm HCl) was added to 48 mL48\ mL of a 0.410 M0.410\ M solution of sodium benzoate (C6H5COONa\rm C_6H_5COONa) the conjugate base of benzoic acid (C6H5COOH\rm C_6H_5COOH Ka=6.6×10−5\rm K_a = 6.6 \times 10^{-5}). Calculate the pH\rm pH of the resulting solution.
An aqueous solution only contains a 0.050 M in a weak base. Which of the following statements would be true about the solution?
Lactic acid, shown below, is added to many beverages, including some sour beers. What is the pH of a 0.050M lactic acid solution in 0.50M hydrochloric acid? (Ka for lactic acid=1.38x10-4)
What is the hydroxide ion (OH-) concentration of a solution with a pH of 6.1?
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H3O+ concentration in diet cola than in milk?
What is the pH of a solution prepared by mixing 50 mL of a 0.10 M HCl solution with 150 mL of pure water?
What is the pH of a 1.1M solution of nitrous acid (HNO2). The Ka of nitrous acid is 7.2 x 10-4
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H3O+ concentration in diet cola than in milk?
Concentration
A solution of LiOH is made by mixing an unknown amount of LiOH with 1 L of water. The pOH is measured to be 3.65, what is the concentration of LiOH?
MW Li: 7 g/mol
MW O: 16 g/mol
pH: Neutralization
A student adds 11.6 mL of a 3.7M KOH solution, to 29 mL of a 1.4 M HCl. What is the final pH after the addition?
To 4.00 L of water was added 100 mg of HF (6.6 x 10-4). What is the pH?
CH3COOH is a weak acid with a Ka of 1.8 x 10-5. In what pH range would you most likely an aqueous solution of Na(CH3COO).
To 150 mL of water was added 0.18 moles of ammonia (NH3 Kb= 2.3 x 10-5) calculate the pH.
Acids and Bases: Henderson Hasselbalch
To a solution of acetic acid (Ka=1.8×10−5\rm K_a = 1.8 \times 10^{-5}) was added 0.1 mol of NaOH\rm NaOH. After the addition of NaOH\rm NaOH the volume was 1.4L and the pH\rm pH was 5.2.
a) This solution a buffer? (True/False)
b) Calculate the number of moles of acetic acid that were originally in solution. Report your answer in moles to three significant figures. Do not include units in the answer field
What is the pH of a solution made by mixing 22g of NaOH in 3.1 L of water?
Molecular formula: Concentration
A solution of HBr has a pOH of 12.2, what is the [H+] concentration?
What is the pH of a solution of 0.1 M sodium acetate (NaCH3CO2) given that the Ka for acetic acid is 1.8×10−5?
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
To a 90 mL90\ mL of 0.17 M0.17\ M of HF\rm HF is added 25 mL25\ mL of 0.06 M0.06\ M NaOH\rm NaOH. The KaK_a of HF\rm HF is 7.2×10−47.2 \times 10^{-4}. Calculate the pH\rm pH of the solution.
What is the pH of pure, neutral water at 37°C? At 37°C, Kw = 2.4x10-14.
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
What is the pH of a solution prepared by mixing 50 mL of a 0.10 M HCl solution with 150 mL of pure water?
The equilibrium constant for the auto-ionization of water at 10 °C is 3.0 x 10-15. What is the concentration of H3O+ ions in pure water at this temperature?
If the pH of pure water is 6.80 at 37 °C, calculate Kw pOH and [OH- ] at this temperature.
Equilibrium: Auto-ionization of water
Given the equilibrium information for water below, what is the concentration of hydroxide ions in a solution of 1.5 M HCl?
2 H2O (l) ⇌ H3O+ (aq) + OH- (aq), Kc = 1x10-14 at 20oC
Equilibrium: ICE Tables and Auto-ionization of Water
Given the equilibrium information for water below, what is the concentration of hydroxide ions in water?
2 H2O (l) ⇌ H3O+ (aq) + OH- (aq), Kc = 1x10-14 at 20oC
If the pH of pure water is 6.80 at 37 °C, calculate Kw pOH and [OH- ] at this temperature.
The compound fluoroacetic acid (shown), has a pKa value of 2.59. What is pKb of its conjugate base?
A solution of [CH3NH3][CH3COO] is made in an undergraduate laboratory. Use the information below to predict the acidity of the solution.
CH3COOH: Ka = 1.8 x 10-5
CH3NH3+: Ka = 2.3 x 10-11
Auto-ionization of Water: pH
If the pH of pure water is 6.80 at 37 °C, calculate Kw pOH and [OH- ] at this temperature.
If an answer has an exponent (ex. 1.6x103), input it as: 1.6e3
The equilibrium constant for the auto-ionization of water at 10 °C is 3.0 x 10-15. What is the concentration of H3O+ ions in pure water at this temperature?
More Titration Problems Questions:
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
Acids and Bases: Titrations
25mL of a solution of 0.5mol/L KOH is required to neutralize 15mL of sulphuric acid. What is the concentration of the acid?
2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(ℓ)2KOH\left(aq\right)+H_2SO_4(aq)\to K_2SO_4(aq)+2H_2O(\ell)
Henderson Hasselbalch: Titrations and pH
For the titration of 50.00 mL of 0.1000 M ammonia (NH3) with 0.1000 M HCl calculate the pH (For ammonia Kb​=1.8×10−5)(For\ ammonia\ Kb​=1.8\times10^{-5})
Before the addition of any HCl
After 20.00 mL of the acid has been added
Redox
A 5.000 mL sample of a solution of hydrogen peroxide, H2O2, was analyzed by titration with potassium permanganate, KMnO4, according to the reaction shown below. The H2O2 sample required 42.8 mL of 0.0175 mol L−1 KMnO4 (aq) to reach the end point.
2 KMnO4 + 5 H2O2 + 6 H+ → 5 O2 + 2 Mn2+ + 2 K+ + 8 H2O
What was the concentration of the H2O2 solution? Choose the closest value.
To a 100 mL of 0.1M of CH3COOH\rm CH_3COOH (acetic acid) is added 25mL of 0.17M NaOH\rm NaOH. The Ka\rm K_a of acetic acid is 1.8×10−51.8 \times 10^{-5}. Calculate the pH\rm pH of the solution. Please report your answer to two decimal places.
25L of a solution of 0.5M KOH is required to neutralize 15L of sulphuric acid. What is the concentration of the acid? Balance the equation if it is unbalanced.
KOH + H2SO4 --> K2SO4 + 2H2O
What volume of hydrochloric acid of 0.1M is required to neutralize 500mL at 0.5M sodium hydroxide?
HCl + NaOH --> NaCl + H2O
Titration Problem
We titrated 40mL of 0.2M HBr with 0.4M NaOH...
The pH meter indicated that the initial pH was 2.9, pH at the half equivalence point was 3.5, equivalence pt was at pH 8.9.
a) What is Ka for HBr?
What volume of 3.16 M H3PO4 solution is necessary to react with 27 mL of 0.18 M Mg(OH)2?
Acid Base Calculation
An impure sample of solid Na2CO3 was reacted with 0.1755 M HCl. A 0.2337 g solid sample required 15.55 mL of HCl solution.
Practice: Long Titration Problem
For the titration of 50.00 mL of 0.1000 M ammonia (NH3) with 0.1000 M HCl calculate the pH
Before the addition of any HCl
After 20.00 mL of the acid has been added
Acids and Bases: Strong Acid Mixture
Practice Question: Strong Base Mixture
Calculate the pH and pOH of a solution containing a mixture of 75.00 mL of 0.100 M HI and 25.00 mL of 0.250 M HClO4.
Buffers: Titration of Sodium Citrate
A student dissolves a sodium citrate (Na3C6H5O7; MW = 258.069 g/mol) tablet in 350.00 mL of water. The student then pipetted 20.00 mL of the solution and performed a titration using a stock solution of HCl previously standardized to a concentration of 0.9899 M. The experiment required 33.55 mL of the HCl solution to reach the endpoint and fully neutralize the sodium citrate solution. Calculate the concentration of the sodium citrate solution.
Titrations
A student prepares a potassium hydrogen phosphate (K2HPO4, MW = 156.1739 g/mol) solution and pipettes 20.00 mL of this solution for a titration. In the titration, it required 23.43 mL of 0.100 M HCl to reach the endpoint. What is the concentration of the potassium hydrogen phosphate solution?
Strong Acids and Bases
Calculate the pH of a basic solution prepared by taking 10.00 mL of 0.700 M NaOH solution and diluting it to 100.00 mL with water.
Titrations
A student prepares a potassium hydrogen phosphate (K2HPO4, MW = 156.1739 g/mol) solution and pipettes 20.00 mL of this solution for a titration. In the titration, it required 17.51 mL of 0.09977 M HCl to reach the endpoint. What is the concentration of the potassium hydrogen phosphate solution?
pH: Neutralization
A student adds 11.6 mL of a 3.7M KOH solution, to 29 mL of a 1.4 M HCl. What is the final pH after the addition?
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
Chemical Reactions: Limiting Reagent
15mL of a 1.2M solution of HCl reacts with 22mL of a 1.4M solution of NaOH. How many moles of NaOH are left after the reaction is complete?
HCl(aq)+NaOH(aq)→H2O(l)+NaCl(aq)HCl_{(aq)}+NaOH_{(aq)}\rightarrow H_2O_{(l)}+ NaCl_{(aq)}
For the titration of 50.00 mL of 0.1000 M ammonia (NH3) with 0.1000 M HCl calculate the pH. Enter 2 decimal places with all answers. Kb=1.8x10-5
Before the addition of any HCl
After 20.00 mL of the acid has been added
Acids and Bases: Titrations
25L of a solution of 0.5M KOH is required to neutralize 15L of sulphuric acid. What is the concentration of the acid? Balance the equation if it is unbalanced.
KOH + H2SO4 --> K2SO4 + 2H2O
Acids and Bases: Titrations
What volume of hydrochloric acid of 0.1M is required to neutralize 500mL at 0.5M sodium hydroxide?
HCl + NaOH --> NaCl + H2O
For which type of titration will the pH be basic at the equivalence point?
A student titrated 10.00 mL of 0.10 M sodium acetate (CH3COONa) with HCℓ and determined that 10.00 mL of HCℓ was needed to reach the equivalence point. At equivalence, what is/are the major species in solution (besides water and any pH-neutral ions)?
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
Henderson Hasselbalch: Titrations
Suppose you performed a potentiometric titration on the solutions in flasks A, B, and C by a gradual addition of HCℓ (aq) to each flask shown.