9.To correctly adjust the pH of a solutionto be used in an electrophoretic separationprocedure, exactly 78.62 mL of 1.209 M NaOH wereadded to 100.00 mL of 1.418 M lactic acid (HLac).HLac + NaOH →NaLac + H₂OPlease answer the following questions.AB.C.Determine the equilibrium concentrationof lactic acid in the buffer solution.MPlease provider your answer below.A← →Check answerDetermine the equilibrium concentrationof NaLac in the buffer solution.Please provider your answer below.2Check answer←→←Given that Ka = 1.403×10-4 for lacticacid, determine the pH of the buffer solution.pH =M

A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

procedure, exactly 78.62 mL of 1.209 M NaOH were added to 100.00 mL of 1.418 M lactic acid (HLac). HLac + NaOH → NaLac + H₂O Please answer the following questions. A B. C. of lactic acid in the buffer solution. M Please provider your answer below. (0) Determine the equilibrium concentration Check answer (0) ← of NaLac in the buffer solution. Please provider your answer below. 0₂ Determine the equilibrium concentration Check answer 仁 → GA 4 FA Given that Ka = 1.403×10-4 for lactic acid, determine the pH of the buffer solution. pH = M

procedure, exactly 78.62 mL of 1.209 M NaOH were added to 100.00 mL of 1.418 M lactic acid (HLac). HLac + NaOH → NaLac + H₂O Please answer the following questions. A B. C. of lactic acid in the buffer solution. M Please provider your answer below. (0) Determine the equilibrium concentration Check answer (0) ← of NaLac in the buffer solution. Please provider your answer below. 0₂ Determine the equilibrium concentration Check answer 仁 → GA 4 FA Given that Ka = 1.403×10-4 for lactic acid, determine the pH of the buffer solution. pH = M

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

Similar questions

need explanation y other options are in correct too
1 2 3 NEXT > A solution is prepared with 0.55 M HNO₂ and 0.75 M KNO₂. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. -2x 0.75 - 2x [0] 0 [0.55-x] 0.55 +x HNO₂(aq) + [0.55] [0.55 + 2x] 0.55 0.55-x Ka = 0.75 [0.75] [0.55 - 2x] H₂O (1) 0.55 + 2x Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. [6.8 x 10-4] [0.75 +x] 6.8 x 10-4 0.55-2x 2 The Ka for this solution of HNO₂ is 6.8 x 10-4. Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the…
#4 Could you circle or make answer visible please.
Calculate the concentration of acid in each buffer solution. The pKa of acetic acid is 4.745
please don't provide handwritten solution..
I'm stuck all those questions need help
all 3 parts please
Determine the Kb for an unknown base by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. NEXT > The pH for a 0.185 M solution of an unknown weak base, B, is 12.95. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) B(aq) + H₂O(1) = OH-(aq) + BH*(aq)
O O O ation.com Overa As strong base is added to a formic acid-sodium formate buffer solution, which of the following will occur? Select all that apply. Check all that apply. More formic acid (HCOOH)will be formed. The added strong base will react with the formate ion (HCOO) in the buffer. More formate ion (HCOO)will be formed. The added strong base will react with formic acid (HCOOH) in the buffer. Do you know the answer? Buffer Google Chrome I know it Think so No Idea 1:04
Only typed solution