A sample of acetic acid is titrated with a standardized NaOH solution. Beyond the end-point of the titration, which of the following must be true? HC,H3O2 (aq) + NaOH (aq) → NaC,H3O2 (aq) + H2O (1) Note: [X] = molar concenctration of X %3D O [H+] > [OH-] [-HO) > [+H] O O [H+] = [OH-]

с $ 4 Micquam Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH₂ (aq) and 0.100 M in NH₂Cl(aq). Consult the table of ionization constants as needed. 11 ApH = Calculate the change in pH when 7.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH = % G Search or type URL 5 A tv 6 9 MacBook Pro & 7 * 00 8 by Machman Learning Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books O ( 9 ) 2 AB O delete

Calculate the pH for each of the cases in the titration of 25.0 mL of 1.50 M pyridine, C5H5N(aq) with 0.500 M HBr(aq) at 25°C. The Kb of pyridine is 1.7×10−9. Report all your answers to 2 decimal places. Record the bold and underlined values to the empty spaces in your handout. Before the addition of any HBr: Question Blank 1 of 5 After the addition of 10.0 mL of HBr: Question Blank 2 of 5 After the addition of 37.5 mL of HBr: Question Blank 3 of 5 After the addition of 75.0 mL of HBr: Question Blank 4 of 5 After the addition of 85.0 mL of HBr: Question Blank 5 of 5

Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 3.00 ✕ 102 mL of solution and then titrate the solution with 0.148 M NaOH. C6H5CO2H(aq) + OH-(aq)  C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2-   M H3O+  M OH-

Create a BCA Table for the Equation: 2HCl(aq) + M(OH)2(aq) --> 2H2O(l) + MCl2(aq) AND FILL OUT THE FOLLOWING SUMMARY. I n this titration, 40.00 mL of 0.0521 M HCl was being neutralized by adding M(OH)2 that had a concentration of approx. 0.07 M. When a total of 11.53 mL of M(OH)2 was added, _____ moles of OH- had been added. Which reacted with the initial _____ moles of H+. After this neutralization reaction, _____ moles of H+ remained in the total volume of _____ mL. This resulted in a calculated pH of _____. The measured pH was 1.86.please answer type in word don't image upload thank you.

Use ICE table and also dont use mmol as your units for stuff

What is the approximate pH at the equivalence point of a weak base-strong acid titration if 50.00 mL of aqueous ammonia (NH3) requires 37.10 mL of 0.1087 mol L-1 HCI? pK₁ =4.75 for ammonia. Report your answer in 2 decimal places.

Calculate the pH of a solution formed by adding 6.00 grams of solid sodium formate, NaCHO₂, to 200.0 ml of 0.400 M formic acid solution, HCHO₂. You may assume that the salt dissolves completely and that the change in volume is negligible upon addition of the solid.pH = ___

The solution started out clear, but when the 12 M HCl was added, lots of the white solid formed. The second round of the eight drops of HCl were added, which produced more white solid taking up most the volume of the test tube. Using the equation and Le Chatelier’s principle, what happened when the HCl was added to the reaction?

A 6.25−g quantity of a diprotic acid was dissolved in water and made up to exactly 275 mL. Calculate the molar mass of the acid if 25.0 mL of this solution required 11.9 mL of 1.00 M KOH for neutralization. Assume that both protons of the acid were titrated.      g/mol