A solution is prepared at 25 °C that is initially 0.36 M in diethylamine ((C,Hs),NH), a weak base with K,-1 ch londe ((CH) NHd). Calculate the pH of the solution. Round your answer to 2 decimal places.
3. (a) Calculate the pH of a solution 0.145 M with respect to CH3CH2COOH and 0.115 M with respect to K+CH3CH2COO-. Ka = 1.3 x 10 – 5 ; pKa = 4.89 (b) Calculate the pH of the same solution after adding 0.015 M KOH. (c) Calculate the pH of the same solution as in part (a) but after addition of 0.015 M HBr.
Calculate the pH of a 0.445 M NH, solution. NH, has a Kb = 1.8 x 10-5. pH = The K, of a weak monoprotic acid is 1.59 x 10-5. What is the pH of a 0.0808 M solution of this acid? pH =
3. Calculate the pH of 0.10 M ammonia, NH) 4. Calculate the pH of 0.10 M KOH. 5. For each reaction, a and b, indicate the acid, base, conjugate acid and conjugate base below each substance. a) NH + H2O = NH3 + OH- b) OH + H₂S = H₂O + HS c) Which substance in the above reactions is amphoteric (amphiprotic
D Question 25 Calculate the pH of a 0.10 M CH3NH,Cl solution. Ky(CH NH) - 4.4x104 5.82 943 Сосоо 4.36 8.18 Question 26 5 pts When a strong acid is added to a strong base in a titration, what is expected at the equivalence point? A acidic solution from the conjugate acid of the strong base A neutral solution with a pH - 7 A acidic solution from the strong acid A basic solution from the strong base A basic...
A buffered solution is made by adding 80.08 NH, Cl to 1.00 L of a 0.65-M solution of NH, Calculate the pH of the final solution (Assume no volume change.) (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 Mind Top Reader. You should not use the OWLv2 References Tables to answer this question as the values will not match.) pl -
NH, is a weak base (Kb = 1.8 x 10-M), so the salt NH, Cl acts as a weak acid. What is the pH of a solution that is 0.033 M in NH CI? pH = pH = {
23. For each solution, calculate the initial pH and the final pH after adding 0.010 mol of HCI. a. 500.0 mL of pure water b. 500.0 mL of a buffer solution that is 0.125 M in HC,H,O, and 0.115 M in NaC,H,O, c. 500.0 mL of a buffer solution that is 0.155 M in CH NH, and 0.145 M in CH NH,CI
NH, is a weak base (Ks = 1.8 x 10-M), so the salt NH Cl acts as a weak acid. What is the pH of a solution that is 0.00M in NH CI? pH
Calculate the pH and concentrations of CH NH, and CH NH; in a 0.0293 M methylamine (CH, NH,) solution. The Kb of CH3NH, is 4.47 x 10-4. pH = [CH, NH] = [CH, NH}=