High School
SAT
ACT
University
MCAT
LSAT
DAT

To a 100 mL of 0.1M of CH_3COOH (acetic acid) is added 25mL of 0.17M NaOH. Th…

Related Topics

Wize University Chemistry Textbook > Buffers and Titrations

Preparing Buffers with Desired pH

1 Activity

Wize University Chemistry Textbook > Buffers and Titrations

Titration Problems

2 Activities

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.
More Preparing Buffers with Desired pH Questions:
Buffer Solutions
Consider a buffer containing 17 grams of sodium acetate (CH3COONa\rm CH_3COONa) and 21g of acetic acid (CH3COOH\rm CH_3COOH) Ka=1.8×10−5\rm K_a = 1.8 \times 10^{-5} in 1L of water.
a) What is the pH\rm pH of this buffer?
b) A graduate student finds a bottle of NaOH\rm NaOH(aq) but the concentration is unknown. To find the concentration the student adds 250mL of the solution to the buffer from part a) and observes a +0.4 change in the pH\rm pH. What is the concentration of the unknown NaOH\rm NaOH?
What are the [H3O+] and pH of a buffer containing 0.25 M propanoate and 0.15 M propanoic acid? (Ka of propanoic acid = 1.3 x 10-5)
pH and Henderson Hasselbalch
How many moles of NaCH3COO should be added to 700mL of a 0.15M of CH3COOH to get a pH of 4.8? Assume no volume change. pKa=4.75
moles of NaCH3COO?
V=700mL (CH3COOH)
Practice: Buffers/Titrations
Buffers and Titrations - Long Answer Practice Problem
A student prepares a buffer solution in the lab by titrating bleach (sodium hypochlorite, NaCℓO) with HCℓ until they produce a 1:1 buffer. Ka for HClO = 3.5 x 10-8.
a. What is the pH of their buffer solution?
Buffers: Citrate Buffer
A student prepares 350.00 mL of 0.186 M sodium citrate (Na3C6H5O7; pKb = 7.60) solution.
a) Calculate the volume (in mL) of 0.150 M HCl required to prepare a citrate buffer with pH = 7 using 25.00 mL of the sodium citrate solution.
b) Calculate the pH of a solution containing 25.00 mL of 0.223 M sodium hydrogen citrate (Na2HC6H5O7) and 25.00 mL of the sodium citrate solution.
Buffers: Preparing a Buffer at Specified pH
Use the following list of chemicals to answer the following questions.
0.50 M HF
0.25 M CH3COONa
Buffer Chemistry
Calculate the volume of 1.10 M NaOH required to prepare a buffer with pH = 9.79 from a 35.00 mL 0.100 M HCN solution (pKa (HCN) = 9.40).
Buffering Action
Determine the volume of 1.00 M BeO required to prepare a buffer with pH of 3.00 using a mixture of 150.0 mL containing 0.0800 M HF and 0.0500 M NaF.
Calculate the pH of a buffer containing 0.100 M HF and 0.250 M NaF after 1.25 mL of 1.30 M NaOH has been added to 75.00 mL of this buffer.
Buffer Chemistry
Calculate the pH of a buffer prepared by adding 1.50 mL of 0.900 M NaOH to 25.00 mL of 0.100 M HCN.
Buffer Chemistry
Calculate the pH of a buffer prepared by dissolving 0.350 g of KCN into 30.00 mL of 0.125 M HCN.
Buffer Chemistry
Calculate the pH of a buffer formed by combining 23.00 mL of 0.250 M HCN with 27.00 mL of 0.150 M KCN.
pKa HCN = 9.40
Buffering Action
Determine the volume of 0.750 M BeO required to prepare a buffer with pH of 5.00 using a mixture of 150.0 mL containing 0.0250 M CH3COOH and 0.0100 M CH3COO- (pKa = 4.75).
Buffering Action
Calculate the pH of a buffer containing 0.200 M HF and 0.150 M NaF after 1.20 mL of 1.25 M HCl has been added to 100.0 mL of this buffer.
Buffer Chemistry
Calculate the volume of 0.100 M NaOH required to prepare a buffer with pH = 9.91 from a 25.00 mL 7.50 x 10-2 M HCN solution (pKa (HCN) = 9.40).
Buffer Chemistry
Calculate the pH of a buffer prepared by adding 2.50 mL of 0.900 M NaOH to 25.00 mL of 0.320 M HCN.
Buffer Chemistry
Calculate the pH of a buffer prepared by dissolving 0.225 g of NaClO into 40.00 mL of 0.750 M HClO.
Buffer Chemistry
Calculate the pH of a buffer formed by combining 17.00 mL of 0.130 M HCN with 33.00 mL of 0.0850 M KCN.
Henderson Hasselbalch: Buffer solutions
A buffer is formed by dissolving 5 g5\ g of sodium benzoate, C6H5COONa\rm C_6H_5COONa, and 6 g6\ g of benzoic acid, C6H5COOH\rm C_6H_5COOH (Ka=6.6×10−5\rm K_a =6.6 \times 10^{-5}) in 1 L1\ L of water.
a) What is the pH\rm pH of this buffer?
b) The buffer is split into two beakers, 500 mL500\ mL each. To the first beaker is added 1 mL1\ mL of 1.0 M1.0\ M HCl\rm HCl and to the second is added 1 mL1\ mL of 1.0 M1.0\ M NaOH\rm NaOH. Calculate the pH\rm pH of each beaker.
Henderson Hasselbalch: Buffer solutions
90 mL90\ mL of 1.4 M1.4\ M HCl\rm HCl was added to 120 mL120\ mL or 1.5 M1.5\ M of bioxalate (HC2O42−\rm {HC_2O_4}^{2-}). The Ka\rm K_a of oxalic acid (H2C2O4\rm H_2C_2O_4), is 5.9×10−25.9 \times 10^{-2}. Calculate the pH\rm pH of the resulting solution.
Buffer solutions
To a solution of acetic acid (Ka=4.0×10−4\rm K_a = 4.0 \times 10^{-4}) was added 0.2 mol0.2\ mol of NaOH\rm NaOH. After the addition of NaOH\rm NaOH the volume was 1.4 L1.4\ L and the pH\rm pH was 4.1.
a) Calculate the number of moles of acetic acid that were originally in solution.
b) (True/False) This solution is a buffer, because pH=pKa±1\rm pH = pK_a \pm 1
Carbonic acid (H2CO3) produces a relatively acidic buffer when combined with it's conjugate base HCO3- (pKa of carbonic acid = 3.6). If a solution of carbonic acid and bicarbonate has a pH of 4.2 what can we say about the relative concentrations of the two components?
An aqueous solution measured to be 0.5 M in sodium acetate and 0.3 M in acetic acid(Ka=1.8×10−5)\left(K_a=1.8\times10^{-5}\right) . Is this a buffer? and what is the pH?
pH and Acid/Base Equilibrium
A buffer is formed by dissolving 10g of sodium benzoate, C6H5COONa\rm C_6H_5COONa, and 12g of benzoic acid, C6H5COOH\rm C_6H_5COOH (Ka=6.6×10−5\rm K_a =6.6 \times 10^{-5}) in 1L of water.
a) What is the pH\rm pH of this buffer? (Two decimal Places)
b) The buffer is split into two beakers, 500mL each. To the first beaker is added 1mL of 1.0 M HCl\rm HCl and to the second is added 1mL of 1.0M NaOH\rm NaOH. Calculate the pH\rm pH of each beaker.
A buffer is prepared by adding 0.021 moles of HI to 250mL of 0.71M of (CH3)2NH(aq). What is the pH of this buffer? Kb((CH3)2NH(aq))=5.4x10-4 (Assume there is no change in volume)
Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5COOH) and 0.15 M sodium benzoate (C6H5COONa). (Ka = 6.5 x 10-5 for benzoic acid)
A buffer is formed by dissolving 5g of sodium benzoate, C6H5COONa, and 6g of benzoic acid, C6H5COOH (Ka =6.5 x 10-5) in 1 L of water.
Buffer Solutions
What are the [H3O+] and pH of a buffer containing 0.25 M propanoate and 0.15 M propanoic acid? (Ka of propanoic acid = 1.3 x 10-5)
Henderson Hasselbalch Equation: pH of Buffer Solutions
Consider 500 mL of a sodium acetate/acetic acid buffer in which the concentration of sodium acetate is 0.50 M and that of acetic acid is 0.10 M. (Ka acetic acid= 1.8×10-5)
(a) What is the initial pH of the buffer?
(b) What is the pH after 100 mL of 0.10 M NaOH is added?
Buffer Solutions
Find the pH of a buffer that consists of 1.0 M sodium phenolate (C6H5ONa) and 1.2 M phenol (C6H5OH). (Ka of phenol = 1x10^-8)
Based on the given ionization constants, which of the following pairs of substances should be dissolved together in water to produce a buffer with pH = 9.85?
AcidKaBaseKbAcetic acid (CH3COOH)1.8×10−5Ammonia (NH3)1.8×10−5Bicarbonate (HCO3−)4.8×10−11Acetate (CH3COO−)5.6×10−10Carbonic acid (H2CO3)4.2×10−7Aniline (C6H5NH2)3.8×10−10Hydrazoic acid (HN3)1.9×10−5Hydrazine (N2H4)8.5×10−7Hydrofluoric acid (HF)6.8×10−4Methylamine (CH3NH2)4.4×10−4Phenol (C6H5OH)1.3×10−10Pyridine (C5H5N)1.5×10−9\def\arraystretch{2} \begin{array}{c|c|c|c} \hline \rm Acid &\rm K_a & \rm Base & \rm K_b\\ \hline \rm Acetic\ acid \ (CH_3COOH) &1.8 × 10^{−5} & \rm Ammonia \ (NH_3) & 1.8 × 10^{−5} \\ \hline \rm Bicarbonate \ (HCO_3^−) & 4.8 × 10^{−11} & \rm Acetate \ (CH_3COO^−) & 5.6 × 10^{−10} \\\hline \rm Carbonic \ acid \ (H_2CO_3) &4.2 × 10^{−7} &\rm Aniline \ (C_6H_5NH_2) & 3.8 × 10^{−10}\\ \hline \rm Hydrazoic \ acid \ (HN_3) &1.9 × 10^{−5} &\rm Hydrazine \ (N_2H_4) & 8.5 × 10^{−7}\\ \hline \rm Hydrofluoric \ acid \ (HF) & 6.8 × 10^{−4}& \rm Methylamine \ (CH_3NH_2) &4.4 × 10^{−4}\\ \hline \rm Phenol \ (C_6H_5OH) & 1.3 × 10^{−10}&\rm Pyridine \ (C_5H_5N) &1.5 × 10^{−9}\\ \hline \end{array}
Let us compare two buffer solutions that you could make from an aqueous solution of the weak acid, HA (aq). In both cases, you start from an identical initial solution. In both buffers, the target buffer ratio is 1A–: 2HA.
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.
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 the expected pH?
Ka of CH3COOH = 1.8×10-5
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.