An initial equilibrium mixture of methyl acetate, water and methyl alcohol contained 4.0 mL of methyl acetate, 3.0 mL of water, and 2.0 mL of methyl alcohol.  Final analysis showed that the solution required 12.15 mL of 0.5000 M NaOH for neutralization.  Calculate  Keq for this hydrolysis experiment.                                                CH3CO2CH3   +   H2O  <---->   CH3CO2H   +   CH3OH   Densities (g/mL):         0.9279                1.000                   1.0530            0.7866 Molar masses.              74.08                  18.01                     60.05             32.04         CH3CO2CH3   +   H2O  <---->   CH3CO2H   +   CH3OH

How do I determine the volume of NaOH delivered and the molar it’s of the standard NaOH?

A chemist adds enough of the theoretical ionic compound MX2 to form a saturated solution. She knows X- is a weak base, so she titrates the solution and finds that [X-] = (1.0x10^-4) M. What is the value for Ksp of MX2 Note: Your answer is assumed to be reduced to the highest power possible.

Calculate the pH of a 1 L solution containing 0.1 M formic acid and 0.1 M sodium formate before and after the addition of 1 ml of 5 M NaOH. How much would be the pH change if the NaOH were added to 1 L of pure water? (pKa formic acid = 3.75)

Solve the first assignment only

+ Base/Acid Ratios in Buffers Just as pH is the negative logarithm of [H3O+]. PK₂ is the negative logarithm of Ka. PK₂ -log Ka The Henderson-Hasselbalch equation is used buffer solutions: calculate the pH of base DAGSK pH =pK₂ +log acid] Notice that the pH of a buffer has a value close to the PK₂ of the acid. differing only by the logarithm of the concentration ratio [base]/[acid]. The Henderson-Hasselbalch equation in terms of pOH and PKb is similar. acid [base pOH = pkt + log- Part A Acetic acid has a K₁ of 1.8 x 105. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: A. [acetic acid] ten times greater than [acetate]. B. [acetate] ten times greater than [acetic acid], and c. [acetate] [acetic acid]. Match each buffer to the expected pH Drag the appropriate items to their respective bins. ▸ View Available Hint(s) [acetic acid] ten times greater than [acetate] pH = 3.74 [acetate] ten times greater than [acetic acid] pH = 4.74 Reset Help…

I did an experiment called Potentiometric Analyses where we titrate NaOH with a solid unknown weak acid.  Our group was told that our weak acid is diprotic. Mass of dry, solid acid = .155g Molar concentration of NaOH (mol/L)= 0.100  Buret reading of NaOH, initial (mL)= 50 mL Buret reading NaOH at stocichiometric point, final (mL)= 22.1 mL Volume of NaOH dispensed (mL) 27.9 mL Moles of NaOH to stoichiometric point (mol) : _____________ (I think the above answer would be 2.79 x 10-2? if yes then skip) Moles of acid (mol) _____________ Molar mass of acid (g/mol) __________ Note: In the book it says for a diprotic acid, 2 mol of OH-, neutralizes one mole of acid.

CONSIDER THE LACTIC ACD BUFFER WITH LACTIC ACID), CH₂CH(OH) COOH AND ITS SALT SODIUM LACTATE, CH₂CH(OH)COo Na t ++₂0= "ott OH OH a) WHAT IS THE PURPOSE OF A BUFFER SYSTEM? 6) WHY IS THE SALT OF THE ACID NEEDED? How DOES THE BUFFER D) HOW DOES THE BUFFER REACT WHEN ACIT) (#30t) IS ADDED: REACT WHEN BASE (OH-) IS ADDED

Question 5 Which is the correct expression for K, for this reaction? Cl2(H2O)8 (s) Cl2 (g) + 8 H2O (g) O K, = (Paı2) (PH20) / (Paı21 120)8) O Kp = 1/ (Pci2) (PH20) %3D O K = (Pa2 (PH20)8 OK, - 1/(Pc20 12013) %3D OK,- (Paz) (Pi 120)

Could someone help me answer these questions? I am unsure on how to go about this.