   # Ion and Net Ionic Equation

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1. Calculate the molecular mass/formula weight for: KHSO3
2. How many of each type of atom are present in 0.667 mol of [CrCl2(NH3)4]Cl
3. Calculate the molecular formula for the compound that contains 40.92% C, 4.58% H,
54.50% O, and has a molecular mass of 176 u.
4. When 1.019 g of potassium reacts with O2, it forms 1.860 g of a rather strange compound. Find the empirical formula of this compound, and explain why it is strange.
5. How many grams of BaSO4 (s) are formed when an excess of BaCl2 (aq) is added to 635 mL of 0.314 M Na2SO4 (aq)?
BaCl2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2 NaCl (aq)
6. Determine the empirical and molecular formulas for:
a. 75.69% C; 8.80% H; 15.51% O; MW = 206
b. 59.0% C; 7.1% H; 26.2% O; 7.7% N; MW = 180

1. Write (a) complete-formula equation, (b) ionic equation, (c) net ionic equation for this neutralization reaction: KHSO4 (aq) + NaOH (aq) → ?
2. In each of the following cases, predict whether a reaction will occur, and, if so, write the net ionic equation for the reaction:
a. ZnSO4 (aq) + BaS (aq) → ?
b. NaHCO3 (aq) + Ca(OH)2 (aq) → ?
3. Assign an oxidation number to each atom in:
a. Al2O3
b. HAsO42c. NaMnO4
4. Identify the reducing agent and the oxidizing agent in the following reaction:
MnO4- + 5 Fe2+ + 8 H+ → Mn2+ + 5 Fe3+ + 4 H2O

1. Balance the equation:
FeS (s) + HCl (aq) → FeCl2 (aq) + H2S (g)
Given 13.2 g FeS and 10.2 g HCl, determine: (a) how much H2S is formed, (b) how much excess reactant is left.

1. Assign the oxidation number to each atom in:

a. Ga2O3
b. H3PO4
c. Ca(MnO4)2
2. 100.00 g of sodium chloride is dissolved in enough water to prepare 10.0 L of solution.
What is the molarity of the solution?
3. Calculate the empirical formula for the compound that contains 40.92% C, 4.58% H, and
54.50% O.
4. Write the (a) complete-formula equation, (b) ionic equation, and (c) net ionic equation for this neutralization reaction: HNO3 (aq) + NaOH (aq) → ?
5. How many grams of BaSO4 (s)

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