find ph in a mixture of: a) 100 mL 0,20 mol/l ch3cooh and 50 ml 0,20...
Part B: A 50.0 mL volume of 0.15 mol L−1 HBr is titrated with 0.25 mol L−1 KOH. Calculate the pH after the addition of 14.0 mL of KOH. Express your answer numerically. Part C: A 75.0 mL volume of 0.200 mol L−1 NH3 (Kb=1.8×10−5) is titrated with 0.500 mol L−1 HNO3. Calculate the pH after the addition of 28.0 mL of HNO3. Express your answer numerically. Part D: A 52.0 mL volume of 0.350 mol L−1 CH3COOH (Ka=1.8×10−5) is...
A 52.0-mL volume of 0.350 mol L−1 CH3COOH (Ka=1.8×10−5) is titrated with 0.400 mol L−1 NaOH. Calculate the pH after the addition of 21.0 mL of NaOH.
Average volume of NaOH used (mL) Concentration CH3COOH in vinegar (mol/L) % CH3COOH in vinegar 5.7 .057 Average volume of NaOH used (mL) Concentration CH3COOH in vinegar (mol/L) % CH3COOH in vinegar 5.7 .057 help???!?!?!?
Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.2400 mol/L butanoic acid, CHCH2CH2COOH (Ka -1.54 x 10-5), with 0.2400 mol/L NaOH solution after each addition of titrant: (a) 0 mL (b) 10.00 ml. pH= (c) 15.00 mL d) 19.00 mLpH- (e) 19.95 mL (1) 20.00 mL (g) 20.05 mL pH= (h) 25.00 mL pH = pH = pH = pH = pH = Be sure to answer all parts. Find the pH...
How to find pH if solutions: 50 ml of 0.1M Na3PO4 + 100 ml of 0.05 M HNO3 20 ml of 0.025 M H2C2O4 + 100 ml of 0.01 M KOH 100 ml of 0.01 M HCl + 10 ml of 0.5 % NH3
Consider the titration of 50 mL of 0.100 M acetic acid (CH3COOH, Ka = 1.8 x 10-5) with 0.200 M NaOH solution. Show all calculations for full credit. a) Write the titration reaction: b) Calculate the pH after 5.00 mL of NaOH: c) Calculate the pH after 12.5 mL of NaOH: d) Calculate the pH after 25 mL of NaOH:
What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the addition of 50 mL of a 0.5 mol/L solution of HCl? 5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the addition of 50 mL of a 0.5 mol/L solution of HCI?
what are the last three values? Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.2400 mol/L butanoic acid, CHjCH2CH2COOH (Ka 1.54 x 10-5), with 0.2400 mo/L NaOH solution after each addition of titrant: (a) 0 mL (b) 10.00 ml. pH= 4.81 (c) 15.00 mL pH = 5.29 (d) 19.00 ml. pH = 6.08 (e) 19.95 mL pH = 7.41 (f) 20.00 mL pH= (g) 20.05 mLpH- (h) 25.00 mLpH- pH = 2.71...
Buffer action 4 A buffer solution consisting of 0.05 mol/L acetic acid (CH3COOH) and 0.05 mol/L acetate (CH3COO-) has been used to buffer a 1 L solution at pH 4.7. A small amount of sodium hydroxide solution containing 0.0001 mol NaOH was added. Which of the following reactions best represents the buffer action? + Select one: O a. NaOH(aq) Na+(aq) + OH(aq) O b. CH3COOH(aq) + H2O(1) CH3COO(aq) H30*(aq) O c. CH3COO(aq) + H2O(0) CH3COOH(aq) OH(aq) O d. CH3COOH(aq) +...
what is the pH of a mixture of 40 ml of 0.100 M HNO3 and 50 ml of 0.100 M NaOH?