
2) You dissolve 15.0 grams of propanoic acid (monoprotic, MW = 74.08 g/mol, Ka = 13x...
Part 2: pH and pOH Calculations 1) You dissolve 0.1500 moles of formic acid (monoprotic, K = 1.8 x 10-) in 2.50 L of water. Calculate the pH of this solution. Use the quadratic formula for this calculation (just to prove you can do it!), i.e., don't use the approximation that x «[...) 2) You dissolve 15.0 grams of propanoic acid (monoprotic, MW = 74.08 g/mol, Ka = 1.3 X 10"") in 95.00 ml of water. Calculate the pol of...
7. A 0.653 g of a monoprotic solid acid (mw= 157 g/mol) is dissolved in water to produce a 50.0 mL solution. The pH of this solution is measure to be pH = 2.13. Determine the ionization constant (Ka) of the acid. 8. A buffer is 0.50 M CH3COOH(aq) and 0.50 M Na(C6H-C00) (aq). For CH2COOH pKa = 4.20 a) Calculate the pH of the buffer solution. b) Calculate the pH after the addition of 40 mL of a 0.150...
7) Calculate the K, of butanoic acid (monoprotic) if a 0.025 M aqueous solution has a pH of 3.21 at 25°C 8) trans-cinnamic acid (C,H,O, monoprotic) has a K = 3.60 x 10-5 a. Calculate the pH of a 0.020 M aqueous solution of this acid. b. Calculate the percentage of acid dissociated (i.e., in the "A" form) in this solution using your calculations in (a). CHEM 120B-Activity #3 Acids and Bases Page 5
A student adds 13.11 grams of propionic acid (a monoprotic acid with molar mass = 74.08 g/mol) to water. When she takes a 25.00 g sample of this solution, and titrates it with 0.1111 M NaOH(aq), she finds that she needs to add 17.17 mL of this solution to reach the endpoint. What was the percent by mass of propionic acid in the solution she made?
1. A weak monoprotic acid has molar mass 180 g/mol. When 1.00 g of this acid is dissolved in enough water to obtain a 300 mL solution, the pH of the resulting solution is found to be 2.62. What is the value of Ka for this acid? 2. A weak monoprotic acid has pKa = 3.08. Calculate the percent ionization of a 0.35 M solution of this acid. 3. Calculate the pH of a solution that is 0.050 M in CH3COOH...
In a flask, you have 40.00 mL of 0.480 M propanoic acid, a weak monoprotic acid with Ka = 1.3 × 10−5. Calculate the pH after the addition of 26.90 mL of 0.480 M NaOH. Report your answer to TWO places past the decimal.
Formic acid Ka: 1.80x10^-4
Propanoic acid Ka: 1.34x10^-5
Chloroacetic acid Ka: 1.36x10^-3
Iodic acid Ka: 1.7x10^-1
What is the pH of a solution that is (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a prepared by dissolving 8.20 g of formic acid (46.03 g/mol) and 10.74 g of sodium formate (68.01 g/mol)...
12.22 g of the monoprotic acid KHP(MW = 204.2 g/mol) is dissolved into water. The sample is titrated with a 0.85 M solution of calcium hydroxide to the equivalence point. What volume of base was used?
7) Calculate the K of butinoic acid (margrotis)ifa 0.025 M aqueous solution has a pH of 3.21 a 25°C. 8) trans-cinnamic acid (C.H.Oz; monoprotic) has a K = 3.60 x 10-5 a. Calculate the pH of a 0.020 M aqueous solution of this acid. ON -OSI b. Calculate the percentage of acid dissociated (ie, in the "A" form) in this solution using your calculations in (a). 0.8 Ho CHEM 120B-Activity #3 Acids and Bases Page 5 of 12
A 50.0 mL sample of 0.21 M propanoic acid, CH3CH2COOH, a weak monoprotic acid, is titrated with 0.11 M KOH. Ka of CH3CH2COOH = 1.4 ✕ 10-5. (a) Calculate the pH at the half-equivalence point. (b) Calculate the pH at the equivalence point.