For the following substances, classify each as either nonelectrolyte or strong electrolyte. 

a. Ca(NO₃)₂
b. NaOH
c. C₆H₁₂O₆
d. NaBr

When a substance with the formula XBr₃ reacts with water, HBr and another acid, H₃XO₃, are produced. H₃XO₃ also contains three acidic hydrogens that react with KOH. After titrating a solution made up of 3.67 g of XBr₃ and 75.0 mL of water, it was discovered that 87.3 mL of 0.132 M KOH were needed to completely neutralize the acid. For the reaction of XBr₃ with water, write a balanced equation.

Identify which of the following ions (Ag⁺, Sr²⁺, and Zn²⁺) are present in the solution given the following data:

1. The addition of sodium chloride to the solution results in a precipitate. The precipitate is filtered off.

2. The addition of potassium sulfate does not result in any precipitate.

3. The addition of sodium carbonate to the solution results in a precipitate.

Write a molecular equation for the following precipitation reactions. If no precipitate forms, write NO REACTION.

1. aluminum sulfate and sodium phosphate

2. chromium (III) nitrate and strontium iodide

3. copper (II) nitrate and lithium phosphate

Identify salt produced by each of the following acid-base reactions.

1. Ca(OH)₂ (aq) + HNO₃ (aq) → 

2. HCl (aq) + Sr(OH)₂ (aq)  →

3. HClO₄ (aq) + Cr(OH)₃ (aq)  →

When sodium hydride is dissolved in water, sodium hydroxide and hydrogen gas are formed. Give the balanced chemical reaction for the reaction.

Consider the following solutions that are combined in the following steps:

Step 1: Initial solution contains 200.0 mL of 0.150 M Ca(OH)₂

Step 2: 100.0 mL of 0.150 M AgClO₄ is added to the solution

Step 3: 100.0 mL of 0.150 M H₂CO₃ is added to the solution

Step 4: 400.0 mL of 0.150 M CH₃NH₂ is added to the solution

Provide the reaction equation that takes place in each step then determine the concentrations of Ca²⁺, OH^–, Ag⁺, ClO₄^–, CH₃NH₂, and CH₃NH₃⁺ in the final solution considering each reaction goes to completion.

Metals can be removed from water by precipitation. 

Ca²⁺ (aq) + Na₂CO₃ (aq) → CaCO₃ (s) + 2 Na⁺ (aq)

Fe²⁺ (aq) + Ca(OH)₂ (aq) → Fe(OH)₂ (s) + Ca²⁺ (aq)

If 1700 L sample of water has 4.0x10^-5 M Ca²⁺ and 8.0x10^-7 M Fe²⁺, calculate the moles of Na₂CO₃ and Ca(OH)₂ needed to precipitate them.

Two acids, HBr and HXO₃, are produced when a compound with a formula of XO₂Br reacts with water. HXO₃ has one acidic hydrogen, which reacts with KOH. A sample of XO₂Br weighing 6.295 g was added to 100.0 mL of water. The solution obtained was titrated with KOH. Determine the atomic mass and identity of the element X if 100.0 mL of 1.000 M KOH is required to neutralize all the acid.

(a) What is the balanced net ionic equation for Sr(OH)₂ + CoCl₃ →

(b) What are the spectator ions?

An aqueous solution of a mixture of salts is suspected to have one or more of these cations: NH₄⁺, Ba^2+, and Fe²⁺. The addition of sodium chloride to the solution does not result in any precipitate. A white precipitate is formed when sodium sulfate is added to the solution. The precipitate is filtered off and sodium carbonate is added to the obtained filtrate. Addition of sodium carbonate to the filtrate results in the formation of a greenish-brown precipitate. Write net ionic equations for the two observed precipitation reactions.

There are multiple possible values of oxidation states for arsenic ranging from –3 to +5. When arsenic is heated in oxygen, tetraarsenic hexaoxide or tetraarsenic decoxide can be produced. What is the formula and oxidation state for each compound?