Predict the products and balance the following reaction: Ag₂SO₄(aq) + NaCl(aq) → A) Ag₂SO₄(aq) + NaCl(aq) → NaSO₄(aq) + AgCl(s) B) Ag₂SO₄(aq) + NaCl(aq) → Na₂SO₄(aq) + 2AgCl(aq) C) Ag₂SO₄(aq) + 2NaCl(aq) → Na₂SO₄(aq) + 2AgCl(s) D) 2Ag₂SO₄(aq) + 4NaCl(aq) → Na₂SO₄(aq) + 4AgCl(s)

Calculate the equilibrium concentration (in M) of PO43− that would be present in a mixture that is originally 0.015 M H3PO4 as well as 0.005 M NaH2PO4, given the following information:     H3PO4(aq)   ↔   H+(aq)   +   H2PO4−(aq)                   Ka1  =  1.5 x 10−5   H2PO4−(aq)   ↔   H+(aq)   +   HPO42−(aq)                 Ka2  =  2.5 x 10−7   HPO42−(aq)   ↔   H+(aq)   +   PO43−(aq)                    Ka3  =  3.5 x 10−9

A reaction occurs between I-(aq) and H2O2(aq) in the presence of H3O+, forming I2(aq) and H2O(l). (1). Write a balanced equation for the reaction.

Given the general equation illustrating the reaction of the acid HA in water, HA (ag) + H2O(1) H3O* (ag) + A (aq)

Write the concentration equilibrium constant expression for this reaction. 312(s)+2 Cr³* (aq)+7H2O(l) →Cr₂O²½˜¯(aq)+61¯ (aq)+14H*(aq) ☑ ==

Complete and balance the following double-displacement chemical equation: ZnCl2(aq) + AgC2H3O2(aq)

2.2 6. (1) Define pH in words. The strong acid HClag has a pH value of 1, use the following equation for a strong acid: Claa HClaa Hog + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H+] (ii) Use the above expression to deduce the pH of HCl (ag) given the concentration of the acid to be 4.5 mol/dm³ pH =

A buffer solution made from nitrous acid and sodium nitrite was titrated with sodium hydroxide. What is the net ionic equation for the reaction?

Which of the following reactions is an acid-base reaction? A) AGNO:(aq) + KF(aq) → AgF(s) + KNO:(aq) B) NH:(aq) + HF(aq) → NH:"(aq) + -F(aq) C) NO: (aq) + AI(s) → NH3(g) + AIO: (aq) D) CH:(g) + 202(g) - 2H:O(g) + CO:(g)