Find the pH of the solution containing 0.04 M Na3PO4. (Ka1= 7x10-3 , Ka2= 2.2x10-7, , Ka3= 4.5x10-13). Note: Write down the equilibrium reaction and state the equilibrium constant

Consider a 1M solution that is prepared using the salt NH4NO. The pK, of ammonia is 4.7 and the pKa of nitric acid is -1.3. Which statements below are accurate about the contents of this solution? • There is more hydroxide than hydronium in the solution at equilibrium. • The solution will have a pH below 7.0 • The solution contains a weak base and an inactive ion. • The solution will have a pH above 7.0. • There is more hydronium than hydroxide in the solution at equilibrium. • The solution contains a weak acid and a strong base. • The solution contains a weak acid and an inactive ion. • The solution contains a weak base and a strong acid.

What is the pH of the buffer that is composed of 0.10 M Na2HPO4 and 0.15 M KH2PO4? (Ka1=7.5 x 103, Ka2=6.20 x 10-8, Ka3=4.8 x 10-13) pH = 7.21 O pH = 7.03 O pH 12.14 O pH = 7.39

9) Rank the following salts in order from most soluble (1) to least soluble (4). CaCrO4, Ksp = 8.0x10-5 CuCl, Ksp= 1.9x107 CaCO3, Ksp = 3.8x10-⁹ BaSO3, Ksp = 8.0x10-6 10) phosphate. Write the dissociation (or dissolution) equation and equilibrium expression, Ksp, for zinc