What is the pH of a solution that contains 0.135 M HCOOH and 0.215 M HCOONa? The pKa of formic acid is 3.750 What is the pH of the solution?

What is the pH of a 0.30 M solution of methylammonium chloride, CH3NH3CL?  What is the concentration of methylamine in the solution?

The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used. (a) What is the concentration of CH3COOH in vinegar? (b) What is the pH of the solution at the end point? (c) What indicator(s) the student should use in this titration? Explain

A new potential cure for the common cold, code-named Z-123, is being tested by a pharmaceutical company. As a research technician, you are told that Z-123 is a monoprotic weak acid, and the company is interested in the drug's Ka value.To find the pKa of Z-123, you prepare a 0.091 mol/L test solution of the drug. The pH of the solution is determined to be 2.77.What is the pKa of Z-123?Express your answer to two decimal places.pKa =   === What is pKb of the conjugate base of Z-123?Express your answer using two decimal places.pKb =

Question 23.c of 23 Submit A 0.5347 g sample of cinnamaldehyde, a compound that contains only carbon, hydrogen and oxygen and has the fragrance of cinnamon was combusted in a flow of excess oxygen. The carbon dioxide collected had a mass of 1.6024 g and the water collected had a mass of 0.2916 g. When cinnamaldehyde was vaporized in a 254.00 mL flask at 100.0 °C and 1.044 bar, the vapour was found to have a mass of 1.1302 g. What amount of hydrogen (H), in moles, is present in the water (H2O) produced? mol 1 3 4 5 6. C 7 8 9. +/- х 100 2. LO

The pH of a 0.0033 M solution of Ca(OH)₂ is

What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of solution? The Ka of acetic acid is 1.8 x 10^-5

Hypochlorous acid, HOCl, is a weak acid having a pKa = 7.46. (a) Show the balanced chemical equation for the hydrolysis of water by OCl- (aq).  (b) Compute the value of pKb for aqueous hypochlorite ion.  (c) If [OCl-] = 0.050 M, then what is the pH of this aqueous solution? (a)     (b)     (c)

What is the pH of a solution that has an H+ concentration of                        (a) 1.75 × 10 –5 mol/L; (b) 6.50 × 10 –10 mol/L; (c) 1.0 × 10 –4 mol/L; (d) 1.50 × 10 –5 mol/L?

Determine the pH of the molecules given in a 1L beaker containing 0.035M solution of the given molecule:  NaNO2,  C6H5CHCOOH, Ba(OH)2. (C6H5CHCOOH, Ka=6.3 x 10^-5, HNO2 Ka= 4.5 x 10^-4, CH3NH2, Kb= 5.0 x 10^-4).