Calculate the pH for both a 0.100 M solution of HClO4 and a 0.100 M solution of a HClO (Ka = 2.9 × 10–8)?
(Don't forget significant figures!)
Calculate the pH for both a 0.100 M solution of HClO4 and a 0.100 M solution...
Calculate the pH of a solution that is 0.0060 M in HClO4 and 0.0060 M in HCN. Ka of HCN is 6.2 × 10−10.
Consider the titration of 50.0ml of 0.300 M NaOH by 0.100 M HClO4-. Calculate the pH of the solution at the following points in the titration: a) no HClO4 added b) 50.0ml of HClO4 added c) 100.0ml of HClO4 added d) 150.0ml of HClO4 added e) 200.0ml of HClO4 added
1. A 0.100 M solution of a weak acid has a pH of 1.96. Calculate the [H3O+] in the solution. 2. Suppose you have a 0.100 M solution of a weak acid that has a pH of 2.07. Calculate the Ka for this acid. *Report your answer to 2 significant figures.
What is the pH of a 2.9 M solution of HClO4? pH = __________?
Calculate the pH of a buffer solution containing 0.100 M CH3COOH and 0.100 M CH3COONa ; Ka of CH3COOH = 1.8 x 10-5
Calculate the pH of a solution that is 0.100 M in hydrofluoric acid (HF) and 0.100 M in sodium fluoride (NaF). Ka of hydrofluoric acid is 6.3 x 10-4
1. Calculate the pH of a 0.0820 M solution of the acid HClO dissolved in water if Ka = 2.9x10-8. 2. Calculate the pH of a 0.4480 M solution of the base H2BO3-1 dissolved in water if Ka = 5.4x10-10 for H3BO3. 3. Calculate the pH of a solution containing the following compounds. (Note that these are concentrations before any reaction occurs). [NaH2PO4] 0.300 M [Na2HPO4] 0.840 M [KOH] 0.054 M 4. For the titration of 15.00 mL of 0.100...
Determine pH, pOH, [H3O+] and [OH-] of a 0.265 M HClO solution. Ka of HClO is 2.9 x 10-8.
What is the ClO- concentration of a mixture that is 0.300 M in HF and 0.100 M in HClO. HF Ka= 6.8*10-4 HClO Ka= 2.9*10-8
Calculate the pH of a mixture when 48.00 mL of 0.100 M NaOH solution is added to 50.00 mL of 0.100 M HCl solution? Write the correct answer in 3 significant figures.