1. For each of the solutions in part 3, calculate an expected pH. The Ka for HC₂H3O2 is: 1.8 x 10⁹ and the Kb for NH3 is 1.76 x 105. Remember to account for the dilution factor. a. 10.0mL of 0.10 M HC₂H₂O₂ + 5.0mL of 0.10M HCI b. 10.0mL of 0.10M NH3 + 5.0mL of 0.10M NaOH c. 10.0mL of 0.10M HC₂H₂O₂ +10.0mL 0.10M NaC₂H₂O₂ d. 10.0mL of 0.10 M NH3 + 10.0mL of 0.10M NH.CI 2. Which solution(s) in question 1 would be considered a buffer solution? 3. Complete the calculation for K, from the earlier discussion of the amphoteric salt. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution. (1) H₂PO4 (aq) + H₂O → H₂O (aq) + HPO42(aq); K₁2 = 6.2 x 10-8 (2) H₂PO4 (aq) + H₂O → H₂PO4(aq) + OH(aq); Kb = = ??? Kw Kal 4. Similarly, the HPO4 ion is also amphoteric. The two possible reactions are: H₂O(aq) + PO4³(aq); Kas = 4.2 x 10-¹3 (1) HPO4 (aq) + H₂O) Kw = → H₂PO4 (aq) + OH(aq); Kb = = ??? K₂2 (2) HPO4 (aq) + H₂O Complete the calculation for Kb. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution.

1. For each of the solutions in part 3, calculate an expected pH. The Ka for HC₂H3O2 is: 1.8 x 10⁹ and the Kb for NH3 is 1.76 x 105. Remember to account for the dilution factor. a. 10.0mL of 0.10 M HC₂H₂O₂ + 5.0mL of 0.10M HCI b. 10.0mL of 0.10M NH3 + 5.0mL of 0.10M NaOH c. 10.0mL of 0.10M HC₂H₂O₂ +10.0mL 0.10M NaC₂H₂O₂ d. 10.0mL of 0.10 M NH3 + 10.0mL of 0.10M NH.CI 2. Which solution(s) in question 1 would be considered a buffer solution? 3. Complete the calculation for K, from the earlier discussion of the amphoteric salt. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution. (1) H₂PO4 (aq) + H₂O → H₂O (aq) + HPO42(aq); K₁2 = 6.2 x 10-8 (2) H₂PO4 (aq) + H₂O → H₂PO4(aq) + OH(aq); Kb = = ??? Kw Kal 4. Similarly, the HPO4 ion is also amphoteric. The two possible reactions are: H₂O(aq) + PO4³(aq); Kas = 4.2 x 10-¹3 (1) HPO4 (aq) + H₂O) Kw = → H₂PO4 (aq) + OH(aq); Kb = = ??? K₂2 (2) HPO4 (aq) + H₂O Complete the calculation for Kb. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: 28. A student prepares 2.00 L of a solution containing 0.440 mol of sodium formate (HCOONa) and…

A: we have to calculate moles of NaOH that must be added to the buffer solution to adjust it's pH to…

Q: A chemist titrates 70.0 mL of a 0.1144M nitrous acid (HNO, solution with 0.2245 M NaOH solution at…

A: Nitrous acid is a weak acid , so when it is titrated with NaOH , it's conjugate base will form . And…

Q: A chemist titrates 200.0 mL of a 0.5292M nitric acid (HNO3) solution with 0.3609M NaOH solution at…

A: Information of question

Q: Classify each of the following samples as a strong acid or a weak acid. Use calculations and/ or…

A: The objective of the question is to classify the acids as weak or strong.

Q: he Ka of acetic acid is 1.8 x 10 -5. Calculate the pH of a solution which is composed of 0.250 M HCH…

Q: 1 Determine the pH of the resulting solutions when the following reagents are mixed. a. 25.00mL of…

Q: Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H502 with 100.0 mL of 0.30 M…

Q: 11. At 25 °C, 4.00 moles of solid C2H5NH3I are dissolved in water to make 2.00 L of solution.…

A: moles of C2H5NH3I = 4.00 molevolume = 2.00 LKb = 5.6010-4Ka = 1.010-14T = 25oC

Q: Which statement is true? I If a solution has a pH of 10.0, there are more H+ ions in this solution…

A: 1) Since pH = -log[H+] Where [H+] = concentration of H+ ions Since more the concentration of H+…

Q: How many grams of CH3COONa must be added to 1.00 L of a 0.100 M CH3COOH solution in order for the pH…

A: The total volume of the solution is 1.00 L. The concentration of CH3COONa in order to have a pH of…

Q: What is the pH of a solution containing a mixture of 0.050 M HC2H3O2 and 0.025 M NaC2H3O2? (Ka =…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: 3. Determine the pH of aqueous of 0.100 M solutions of the following salts. The provided K₂ and Kb…

A: The answer to the following question is-

Q: Acetic acid is a weak monoprotic acid with K₂ = 1.77 x 10-5. NaOH(s) was gradually added to 1.00 L…

Q: Calculate the equilibrium constant (Ka) for this acid.

A: Given 0.10 M formic acid is put in water, 4.15% dissociates to form formate ion and hydronium ion.

Q: 1. Calculate the change in pH when 5.00 mL of 0.0100 M HNO3 is added to 50.0 mL of water. 2. Write…

A: 1) Given, V1 = 5 mL = 5 × 10-3 L M1 = 0.0100 M Molarity, M = number of moles / volume in L,…

Q: 16. The Ka of Hydrocyanic acid is 4.9 X 10-10 Consider a 0.050 M solution of its salt potassium…

A: To Find: To find the pH value of the salt solution.

Q: Calculate the pH of a 0.12 M solution of NaC2H3O2 (for HC2H3O2 Ka= 1.8 x 10 ^-5). A. 5.09 B. 8.91…

A: Answer:When salt of weak acid and strong base is added in water it gets hydrolyzed to produce OH-…

Q: Let H2A represent a diprotic acid and let A² represent its corresponding base. A 40.0 mL sample of…

A: Diprotic acid is an acid that can give two hydrogen ions (H+) or protons per molecule in an aqueous…

Q: Calculate the pH of a buffer solution prepared by dissolving 0.83 mole of acid, HA, and 0.67 mole of…

A: Given data is as follows: The number of moles of HA acid = 0.83 mol The of moles of salt NaA = 0.67…

Q: A mixture of acids is made that has 0.0500 M HNO3 and 0.0300 M HC₂H302. The K₂ for HC₂H3O₂ is 1.8 x…

A: The concentration of HNO3 is 0.0500 M.The concentration of HC2H3O2 is 0.0300 M.The Ka of HC2H3O2 is…

Q: 1. Write a chemical equation for the dissociation of the hypochlorite ion, ClO-1, in water to make a…

A: Hello. Since the question contains multiple parts, the first part is solved. In case the solution…

Q: Calculate the pH of a solution formed by mixing 300.0 mL of 0.15 M NH4CI with 400.0 mL of 0.20 M…

A: Given: Concentration of NH4Cl = 0.15 M Volume of NH4Cl solution added = 300.0 mL = 0.300 L…

Q: b) c) Why do these two solutions 3. Complete the following table. Be sure to show each cal pKa…

Q: What is the pH of a solution containing a mixture of 0.050 M HC2H3O2 and 0.025 M NaC2H3O2? (Ka =…

A: Using fomula of pH of buffer solution we can solve this problem.

Q: 0.002 grams of an alkaline earth metal-hydroxide salt was added to 50 mL of DI water and allowed to…

A: Mass of alkaline earth metal-hydroxide salt = M(OH)2 = 0.002 g Volume of water = 50 mL = 0.050 L…

Q: Let HA represent a weak acid. A 27.5 mL sample of 0.20 M HA was titrated with 0.25 M NaOH. The…

Q: A 10.0 mL solution of 0.330 M NH3 is titrated with a 0.110 M HCl solution. Calculate the pH after…

Q: 11. Calculate the concentrations of all species present in a 0.416 M H3PO4 solution. Ignore the auto…

A: When a weak acid dissociates to form H+, it attains equilibrium after some time. The equilibrium…

Q: Let HA represent a weak acid. A 10.0 mL sample of 0.60 M HA was titrated with 0.30 M NaOH. The…

A: The pH of a weak acid and dissociation constant (Ka) are related by the following Henderson…

Q: Consider the following: HNO2 + NaOH => H20 + NaNO2 50.0 mL of 0.200 M nitrous acid (HNO2…

A: The given chemical reaction is: HNO2 + NaOH → H2O + NaNO2 The given information is: Volume of…

Q: Which statement is true? I If a solution has a pH of 12.0, there are more H+ ions in this solution…

A: 1) Since the pH of pure water = 7 And since pH = -log[H+] where [H+] = concentration of H+ ions…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

1. For each of the solutions in part 3, calculate an expected pH. The Ka for HC₂H3O2 is: 1.8 x 10¹5
and the Kb for NH3 is 1.76 x 10. Remember to account for the dilution factor.
a. 10.0mL of 0.10 M HC₂H₂O2 + 5.0mL of 0.10M HCI
b. 10.0mL of 0.10M NH₂ + 5.0mL of 0.10M NaOH
c. 10.0mL of 0.10M HC₂H₂O₂ +10.0mL 0.10M NaC₂H₂O₂
d. 10.0mL of 0.10 M NH3 + 10.0mL of 0.10M NH₂CI
2. Which solution(s) in question 1 would be considered a buffer solution?
3. Complete the calculation for K, from the earlier discussion of the amphoteric salt. Will this ion
be acidic or basic? Predict the expected pH for the 0.050M solution.
(1) H₂PO4 (aq) + H₂O
→ H3O*(aq) + HPO42(aq); Ka2 = 6.2 x 10-8
(2) H₂PO4 (aq) + H₂O
→
Kw
H3PO4(aq) + OH(aq); Kb = ???
Kal
4. Similarly, the HPO4 ion is also amphoteric. The two possible reactions are:
(1) HPO4² (aq) + H₂O → H3O*(aq) + PO4³(aq); Kas = 4.2 x 10-¹3
(2) HPO4 (aq) + H₂O
Kw
→ H₂PO4 (aq) + OH(aq); Kb =
<= ???
K₁2
Complete the calculation for Kb. Will this ion be acidic or basic? Predict the expected pH for the
0.050M solution.
(OVER)
53

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Calculate the pH of a solution formed by mixing 300.0 mL of 0.15 M NH4C1 with 400.0 mL of 0.20 M NH3. The Kþ for NH3 is 1.8 × 10-5. a. 6.22 O b.8.76 OC. 4.74 O d.9.51 O e. 9.01
17. Find the pH of 0.3500 M HNO₂(ag) solution @ 25 °C. K, for HNO₂ = 4.6 x 10-4 HNO₂ + H₂O NO₂ + H₂O+ A. 4.79 B. 3.79 C. 6.55 D. 8.72 18. What is the percent ionization of a 3.34 M solution of nicotinic acid, HC6H4NO₂? (K₂ = 1.4 x 10-5 @ 25 °C) HC6H4NO₂ + H₂O C6H4NO₂ + H₂O+ A. 4.68% B. 6.84 % C. 0.2% D. 48.8%
5. Determine the pH of the resulting solutions when the following reagents are mixed. a. 20.00mL of 0.2500M HCI mixed with 35.00mL of 0.2250M NaOH b. 18.00mL of 0.3500M HC₂H3O2 mixed with 15.00mL of 0.3000M NaOH c. 22.50mL of 0.2000M NH3 mixed with 25.00mL of 0.1000M HCI d. 25.00mL of 0.1000M HClO₂ mixed with 25.00mL of 0.1000M KOH e. 15.00mL of 0.1000M CH3NH₂ mixed with 25.00mL of 0.1500M HCI
5. Determine the pH of the solution which has 10% of NaOH in deionized water by mass. The NaOH which was used to prepare 10% solution has a density of 1.131kg/L. Assumption: 100 % dissociation. N2OH + Na* + OH
17. Determine the pH of the resulting solutions when the following reagents are mixed. a. 20.00mL of 0.2500M HCI mixed with 35.00mL of 0.2250M NaOH b. 18.00mL of 0.3500M HC2H;O2 mixed with 15.00mL of 0.3000M NaOH 22.50mL of 0.2000M NH, mixed with 25.00mL of 0.1000M HCI d. 25.00mL of 0.1000M HCIO, mixed with 25.00mL of 0.1000M KOH e. 15.00mL of 0.1000M CH3NH2 mixed with 25.00mL of 0.1500M HCI
1. calculate the pH of a solution obtained by mixing 30.4 mL of 0.03 M HCL with 31.4 mL of o.1 M HNO3 solution 2.A given weak acid has a pKa of 8.27. Calculate the percent ionized in 0.34 M of the weak acid. 3. Calculate the pH of 0.021 M Sr(OH )2 PLEASE DO ALL THREE
Calculate the pH of each of the following solutions a. 0.10 M propanoic acid, CH3CH2COOH, Ka = 1.3 x 10-5 b. 0.10 M sodium propanoate, NaCH3CH2COO. c. A mixture containing 0.10 M propanoic acid and 0.10 M sodium propanoate d. Calculate the pH after 0.020 mole of HCl is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate e. Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate
b. I'm falling asleep.... The CO₂ concentration in a classroom can increase over the lecture period due to poor ventilation. You decide to measure the pH of pure water in contact with the atmosphere as an indirect way to determine whether you have adequate ventilation. You measure a pH value of 5.3. Assuming equilibrium, i. What is the concentration of CO2 in the classroom? ii. How does the value you calculated compare to the recommended safe level of 800-1000 ppm?
10 11 12 13 14 15 16 17 18 19 20 A chemist titrates 170.0 mL of a 0.3333 M nitric acid (HNO, solution with 0.1703M NaOH solution at 25 °C. Calculate the pH at equivalence. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the soluțion equals the initial volume plus the volume of NaOH solution added. pH = %3D Submi Continue MacBook Air
What is the pH of a solution that results when 0.010 mol HNO 3 is added to 500. mL of a solution that is 0.10 M in aqueous ammonia and 0.50 M in ammonium nitrate. Assume no volume change. (The K b for NH 3 = 1.8 × 10 –5.) a. 5.05 b. 8.44 c. 10.07 d. 9.26 e. 8.67
18. A. Calculate [OH−] for this strong base solution: 7.3×10−2 M KOH and then it's pH B. Calculate [OH−] for this strong base solution: 10.0 mL of 1.00×10−2 M Ca(OH)2 diluted to 500.0 mL and it's pH C. Calculate [OH−] for the strong base solution formed by mixing 10.0 mL of 1.50×10−2 M Ba(OH)2 with 34.0 mL of 6.0×10−3 M NaOH and it's pH
A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa? Ka-1.80x10-4. The total volume is 1.00L. What is the pH of this solution? O a. 0.398 O b. 4.143 O c. 10.653 O d. 9.857 O e. 3.347