You are asked to estimate the pH of a 15mL of 0.09 N of HCl when 16.9mL of 0.085 N NaOH is added to the solution. Your supersaver informed you that she added 100mL of diluent."

5 What volume, in milliliters, of 0.240 M NaOH should be added to a 0.135 L solution of 0.030 M glycine hydrochloride (p Kal = 2.350, pKa2 = 9.778) to adjust the pH to 2.78? 5 NaOH volume = mL

Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 299 mL 0.0611 M 3‑(?‑Morpholino) propanesulfonic acid (MOPS) to give the solution a pH of 7.55. The p?a of MOPS is 7.18. NaOH volume= mL

10 11 12 13 14 15 16 17 18 19 20 21 22 A chemist titrates 180.0 mL of a 0.4289 M pyridine (C,H,N) solution with 0.5274M HCI solution at 25 °C. Calculate the pH at equivalence. The p K, of pyridine is 8.77. Round your answer to 2 decimal places. d- Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. PH = %3D Submit Assignment Continue MacBook Air F12 F10 F9 F8 F7 000 000 * ES F6 F4 esc F2 F3 F1 & *

Classify the following solutions as one of these types AND calculate the pH: strong acid, strong base, weak acid, weak base, buffer, neutral salt. a) 0.040 M NaF (Ka for HF = 7.2 x 10-4) b) 10 M HClO4 c) A solution made by mixing 10.0 mL of 0.072 M NaOH with 15.0 mL of 0.100 M acetic acid (pKa for acetic acid = 4.75) d) 0.453 M NaCl

A chemist titrates 100.0 mL of a 0.4364 M dimethylamine ((CH3)2NH) solution with 0.1921 M HCl solution at 25 °C. Calculate the pH at equivalence. The pk of dimethylamine is 3.27. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCI solution added. pH = -0 §

It says that my answers are wrong but it won’t tell me what answers are wrong I thought I did it right please help me.

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

Calculate the pH of a solution formed by adding 2.00 grams of solid potassium cyanide, KCN, to 180.0 ml of 0.340 M hydrocyanic acid solution, HCN. You may assume that the salt dissolves completely and that the change in volume is negligible upon addition of the solid.

How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.396 M hypobromous acid, HBrO, to form a buffer solution of pH 8.95? The Ka of HOBr is 2.0 × 10–9. Express your answer in moles using at least three significant figures. Do not use scientific notation.