Consider three solutions A – C of the following substances, all at a total or initial concentration of 0.100 M. Which of the following statements are true? Select all that apply. A H3PO4(aq)B NaH2PO4(aq) C Na2HPO4(aq)   Solution A has the lowest pH. In solution B, dissolved H2PO4– cannot act as a Brønsted acid. Solution C has the lowest pH.  In all solutions, the concentration of hydroxide ion is lower than 0.100 M at equilibrium. Solution A contains a negligible amount of H3PO4 at equilibrium.  Solution C contains a negligible amount of H3PO4 at equilibrium.

Calculate the [H3O^+] and the pH of each polyprotic acid solution. Please explain. A) 0.125 M H2CO3 B) 0.125 M H3C6H5O7

Write separate equations representing the reaction of H2 PO4−(a) as a base with HBr(b) as an acid with OH−

Original concentration of Acetic Acid was 0.1033 M and NaOH was 0.1104 M there is part a done, need to do part B

30 mL of 0.25 mol L' HNO3(aq) is placed in a flask and titrated with 0.25 mol L NaOH(aq) solution. What is the pH of the solution in the flask when 25 mL of the NaOH(aq) solution has been added? Answers A - D A 4.64 B 1.38 C 7.00 D 1.64

What concentration of KNO2 must be added, at 25 degrees Celsius, to 0.50 M HNO2 to result in a solution whose pH is 3.49?

The pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a/ Determine the concentration of [OH-] in the solution.  b/ Write the expression for the Kb of NaCH3COO (aq) and calculate its values.  c/ Calculate the pKa of CH3COOH. d/ HCl (aq) is added to 1.00 L solution of 1.00 M NaCH3COO (aq). Write the chemical reaction between HCl (aq) and NaCH3COO (aq).  e/ How many mol of HCl (aq) is needed to make a buffer solution with pH = 5.00 from 1.00 L of 1.00 M NaCH3COO (aq).

What word is used to describe a chemical that can behave like an acid OR a base? amphoteric a salt isoprotic hydorphillic or none of these words