Calculate the pH of the solution obtained by titrating 40 ml of 0.35 M HNO3(aq) with 0.4 M NaOH(aq) to the equivalence point. Take K = 4.6x10^M.
A) calculate the ph of a 0.028 M HNO3 solution B) Calculate the pH of a 0.028 M solution of benzoic acid (Ka=6.5x10^-5)
Calculate the pH of a 1.260 M solution of HNO3.
A. Calculate the pH of a 0.0001 M HNO3 solution B. Calculate the pH of 0.08 M Sr(OH)2 solution C. Calculate the pH of a 0.02 M hydrazoic acid solution (HN3 ----> (H+) + (N3-)), pKa = 4.72 D. Aluminum carbonate (AI2(CO3)3) reacts with phosphoric acid(H3PO4) to produce aluminum phosphate (AIPO4), carbon dioxide, and water 1. Write a balanced equation for the reaction 2. Calculate the mass of phosphoric acid (g) required to react with 100 g of an aluminum...
Calculate pH of 0.25 M HClO (aq) Calculate pH of 0.15 M CH3 NH2 (aq)
Calculate the pH of a mixture that contains 0.18 M of HNO3 and 0.27 M of HC6H5O. Please show me how to do this! I'm not sure how to solve for the pH when given two substances. Thanks!
Calculate the pH of a solution formed by mixing 50.00 mL of 0.0100 M HNO3 with 30.00 mL of 0.0150 M solution of Ba(OH)2
2) a) Calculate the change in pH when 8.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). delta pH= ? b) Calculate the change in pH when 8.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution. delta pH= ?
the HNO3 concentration in a raindrop was measured to be 4.5x10^-4 M. Calculate the pH of this raindrop.
5. Calculate the pH of 0.20 M Ba(OH)2 (aq) and 0.20 M NaOH (aq). Should they be the same? Why or why not?