1a. A buffer solution is prepared by mixing 15.0 mL of 2.00 M Acetic Acid and...
1a. A buffer solution is prepared by mixing 15.0 mL of 2.00 M Acetic Acid and 10.0 mL of 1.50 M NaC2H3O2. Determine the pH of the solution after the addition of 0.01 moles NaOH (assume there is no change in volume when the NaOH is added). Ka HC2H3O2 = 1.80E-5
1b. A buffer solution is prepared by mixing 55.0 mL of 1.15 M HF and 99.0 mL of 0.450 M NaF. Determine the pH of the solution after the addition of 0.015 moles HCl (assume there is no change in volume when the HCl is added). pKa HF = 3.167
1c. A buffer solution is prepared by mixing 22.0 mL of 1.45 M HF and 25.0 mL of 2.45 M NaF. Determine the pH of the solution after the addition of 0.015 moles HCl (assume there is no change in volume when the HCl is added). Ka HF = 6.8E-4
Homework Answers
Add Answer to:
1a. A buffer solution is prepared by mixing 15.0 mL of 2.00 M
Acetic Acid and...
A buffer solution is prepared by mixing 15.0 mL of 2.20 M Acetic Acid and 30.0...
A buffer solution is prepared by mixing 15.0 mL of 2.20 M Acetic Acid and 30.0 mL of 1.55 M NaC2H3O2. Determine the pH of the buffer. pKa HC2H3O2 = 4.745 pH:_____
A buffer solution is prepared by mixing 150 ml of 2.20 M Acetic Acid and 300...
A buffer solution is prepared by mixing 150 ml of 2.20 M Acetic Acid and 300 mL of 1.5 H is added CHO. Debermine the pot the solution after the addition of 0.01 moles NOH (sume there is no chang BK HCl 0,445
5) A 1 L buffer solution is 0.520 M in HF and 0.520 M in NaF....
5) A 1 L buffer solution is 0.520 M in HF and 0.520 M in NaF. Calculate the pH of the solution after adding 0.220 moles of NaOH. Assume no volume change upon the addition of a base. Ka for HF is 3.5 X 10-4
A buffer is prepared by mixing 75.0 mL of 0.40 M aqueous HF and 25.0 mL...
A buffer is prepared by mixing 75.0 mL of 0.40 M aqueous HF and 25.0 mL of 0.80 M aqueous NaF. At 25oC, Ka = 3.5 x 10-4 for HF. SHOW WORK (a). (4 points) Calculate the pH of the buffer. (b). (4 points) Your instructor accidentally dropped the bottle containing the buffer in part (a) in a bucket of water, that initially contained 4.00 L of water. What is the pH of the resulting solution?
1. Calculate the pH of a buffer solution prepared by mixing 0.250 L of 0.150 M...
1. Calculate the pH of a buffer solution prepared by mixing 0.250 L of 0.150 M acetic acid with 0.200 L of 0.250 M sodium acetate. Ka acetic acid = 1.8 x 10-5 Calculate the pH of this solution of after the addition of 0.003 L of 0.200 M HCL 2. Consider a buffer solution prepared by mixing 0.250 L of 0.150 M acetic acid with 0.200 L of 0.250 M sodium acetate. Ka acetic acid = 1.8 x 10-5...
A 1.32 L buffer solution consists of 0.121 M butanoic acid and 0.345 M sodium butanoate....
A 1.32 L buffer solution consists of 0.121 M butanoic acid and 0.345 M sodium butanoate. Calculate the pH of the solution following the addition of 0.066 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The Ka of butanoic acid is 1.52 × 10-5. A 1.44 L buffer solution consists of 0.326 M propanoic acid and 0.103 M sodium propanoate. Calculate the pH of the solution following the addition of...
In this problem you will predict the pH of a buffer solution and then predict the...
In this problem you will predict the pH of a buffer solution and then predict the new pH after you add NaOH or HCl. Write your answers to three decimal places (X.XXX). The Ka of HC2H3O2 is 1.8×10−51.8×10−5. 1) Calculate the pH of a buffer made from mixing 11.011.0 mL of 0.080.08 M NaC2H3O2 and 9.29.2 mL of 0.080.08 M HC2H3O2. 2) Calculate the pH of the buffer when 5.25.2 mL of 0.0090.009 M NaOH is added to the buffer...
A buffer is prepared by adding 0.250 mol of NaF to 1.00L of 0.100 M HF....
A buffer is prepared by adding 0.250 mol of NaF to 1.00L of 0.100 M HF. Calculate the pH of the resulting solution. Use Ka value of 7.2× 10^4 How many moles of NaOH must be added to this buffer solution to change the pH by 0.38 units?
Consider 1.0 L of a solution which is 0.80 M HF and 0.55 M NaF (K...
Consider 1.0 L of a solution which is 0.80 M HF and 0.55 M NaF (K for HF - 7.2x104). Part 1 Calculate the pH of this solution. pH- Part 2 Calculate the pH after 0.10 mol of HCl has been added to the original buffer solution. Assume no volume change on addition of HCI. pH- Part 3 Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition...
You prepared a phosphate buffer solution by mixing 40.0 mL of 0.250 M KH_2PO_4 and 60.0...
You prepared a phosphate buffer solution by mixing 40.0 mL of 0.250 M KH_2PO_4 and 60.0 mL ol 0.450 M K_2HPO_4 solution. (a) What are the molar concentrations of H_2PO_4 and HPO_4^2-, respectively, in the final buffer solution? (b) Calculate the pH of the solution. (c) Write a net ionic equation when a strong acid, such as HCl(aq) is added to the phosphate buffer solution. (d) Calculate the final pH when 0.0060 mol of HCl is added to the buffer...
A buffer solution is prepared by mixing 150 ml of 2.20 M Acetic Acid and 300 mL of 1.5 H is added CHO. Debermine the pot the solution after the addition of 0.01 moles NOH (sume there is no chang BK HCl 0,445
1. Calculate the pH of a buffer solution prepared by mixing 0.250 L of 0.150 M acetic acid with 0.200 L of 0.250 M sodium acetate. Ka acetic acid = 1.8 x 10-5 Calculate the pH of this solution of after the addition of 0.003 L of 0.200 M HCL 2. Consider a buffer solution prepared by mixing 0.250 L of 0.150 M acetic acid with 0.200 L of 0.250 M sodium acetate. Ka acetic acid = 1.8 x 10-5...
Consider 1.0 L of a solution which is 0.80 M HF and 0.55 M NaF (K for HF - 7.2x104). Part 1 Calculate the pH of this solution. pH- Part 2 Calculate the pH after 0.10 mol of HCl has been added to the original buffer solution. Assume no volume change on addition of HCI. pH- Part 3 Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition...
You prepared a phosphate buffer solution by mixing 40.0 mL of 0.250 M KH_2PO_4 and 60.0 mL ol 0.450 M K_2HPO_4 solution. (a) What are the molar concentrations of H_2PO_4 and HPO_4^2-, respectively, in the final buffer solution? (b) Calculate the pH of the solution. (c) Write a net ionic equation when a strong acid, such as HCl(aq) is added to the phosphate buffer solution. (d) Calculate the final pH when 0.0060 mol of HCl is added to the buffer...
Most questions answered within 3 hours.
-
What are some specific reasons behind aquatic life migration and
provide 2 examples
asked 4 minutes ago -
Add appropriate descriptive comments to EACH line of the
code in the project explaining why the...
asked 5 minutes ago -
Finding Probabilities in Normal
Distributions
A manufacturer produces items whose lengths are normally
distributed with a...
asked 10 minutes ago -
Radioisotopes are often used in medical imaging, however are
not something we want to linger in...
asked 14 minutes ago -
A shipment of 10,000 bags of oranges arrives at a distribution
center with a nominal weight...
asked 15 minutes ago -
If you found out how many people in four different age groups
preferred each of the...
asked 15 minutes ago -
If your unknown compound is water soluble but does not change
the pH of the water,...
asked 32 minutes ago -
Background:
“Belinda!” called Kyle, running to catch up to her. Belinda
turned around and waited for...
asked 31 minutes ago -
Assume that a firm earns revenue according to R(Q)=a+bQ+cQ^2.
Marginal revenue is equivalent to the first...
asked 32 minutes ago -
6. Violations of the factor-endowment theory of
trade
While different natural resources and the theory of...
asked 43 minutes ago -
An even thick log was supported at a point whose distance from
one end was 2.00...
asked 42 minutes ago -
why is being able to work in teams / collaboration important for
your future career? Provide...
asked 48 minutes ago