Calculate the pH of the solution that results from each of the following mixtures.
1. 50.0 mL of 0.15 molL−1 HCOOH (Ka=1.8×10−4) with 80.0 mL of 0.13 molL−1 HCOONa
2. 125.0 mL of 0.11 molL−1 NH3 (Kb=1.76×10−5) with 240.0 mL of 0.11 molL−1 NH4Cl
Express your answer using two decimal places.
Calculate the pH of the solution that results from each of the following mixtures. 1. 50.0...
Calculate the pH of the solution that results from each of the following mixtures. A) 55.0 mL of 0.15 molL−1 HCOOH (Ka=1.8×10−4) with 80.0 mL of 0.13 molL−1 HCOONa. B) 135.0 mL of 0.13 molL−1 NH3 (Kb=1.76×10−5) with 240.0 mL of 0.13 molL−1 NH4Cl
Calculate the pH of the solution that results from each of the following mixtures. Part A 55.0 mL of 0.17 molL−1 HCOOH (Ka=1.8×10−4) with 80.0 mL of 0.12 molL−1 HCOONa Express your answer using two decimal places. pH = ??
Calculate the pH of the solution that results from each of the following mixtures. a.) 50.0 mL of 0.15 M HCHO2 with 80.0 mL of 0.13 M NaCHO2 pH_____ b.) 125.0 mL of 0.12 M NH3 with 250.0 mL of 0.12 M NH4Cl pH____
Calculate the pH of the solution that results from each of the following mixtures. A. 55.0 mL of 0.15 M HCHO2 with 75.0 mL of 0.13 M NaCHO2 B. 135.0 mL of 0.13 M NH3 with 260.0 mL of 0.13 M NH4Cl
Calculate the pH of the solution that results from each of the following mixtures. 55.0 mL of 0.15 M HCHO_2 with 70.0 mL of 0.13 M NaCHO_2 120.0 mL of 0.13 M NH_3 with 260.0 mL of 0.13 M NH_4C1
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak acid. 3. Calculate the pH of a...
Use the Henderson-Hasselbalch equation to calculate the pH of each solution: (a) a solution that is 0.20 M in HCHO2 and 0.10 M in NaCHO2. (Ka=1.8×10−4) (b) a solution that is 0.14 M in NH3 and 0.19 M in NH4Cl. (Kb=1.76×10−5)
Determine the pH of each of the following solutions. Part A 0.11 molL−1 NH4Cl Express your answer to two decimal places. Part B 0.15 molL−1 CH3COONa Express your answer to two decimal places. Part C 0.13 molL−1 NaCl Express your answer to two decimal places.
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 12.0 mL of KOH. Express your answer numerically. A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 13.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 33.0 mL...
1. What is the pH of a buffer consisting of 0.30 M CH3COOH & 0.20 M NACH:COO? Ka= 1.8 x 10-5 2. What is the pH of the buffer with 0.10 M NH3 and 0.20 M NH4NO3? Kl = 1.8 x 10-5 3. What is the pH of a buffer formed from combining 10 mL of 0.250 M HCl with 90 mL of 0.150 M NH3? (K = 1.8 x 10-) 4. Calculate the pH of the solution that results...