For the reactions in the earlier exercise , write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write "No reaction."

For the reactions from two exercies above, write the balanced molecular equation, complete ionic equation, and net ionic equation. If no precipitate forms, write "No reaction."

Write a formula equation, a total ionic equation, and a net ionic equation for the reaction of iron and silver nitrate solution.

Write the balanced net ionic equation for the reaction of $\mathrm{HF}$ and $\mathrm{LiOH}$.

For each reaction, write an overall, balanced equation and the net ionic equation.
(a) the reaction of aqueous lead(II) nitrate and aqueous potassium hydroxide

$$\ce{2HBr(aq) + Na2CO3(aq)->H2O(l) + CO2(g) + 2NaBr(aq)}$$

Write the complete ionic equation and identify all of the phases in your answer. Then write the net ionic equation and also identify all of the phases in your answer.

Write balanced complete ionic and net ionic equations for the following reaction:

$$\mathrm{HI( a q )+KOH( a q )→ H_2O( l )+KI( a q )}$$

Express your answer as a complete ionic equation. Identify all of the phases in your answer. Express your answer as a net ionic equation.

Write balanced equations for the reactions between the following. calcium carbonate and hydrobromic acid. Write the net ionic equation for the reaction.

Differentiate between the formula equation, the complete ionic equation, and the net ionic equation. For each reaction in Question 6, write all three balanced equations.

Write balanced, complete, ionic, and net ionic equations for each of the following reactions.

1. Write balanced complete ionic equation for the reaction:

$$\ce{CaS(aq) \ + CuCl_2(aq) -> CuS(s) + CaCl_2(aq)}$$

2. Write balanced net ionic equation for the reaction:

$$\ce{CaS(aq) + CuCl_2(aq) -> CuS(s) + CaCl_2(aq)}$$

3. Write balanced complete ionic equation for the reaction:

$$\ce{NaOH(aq) + HNO_3(aq) -> H_2O(l) + NaNO_3(aq)}$$

4. Write balanced complete ionic equation for the reaction:

$$\ce{2K_3PO_4(aq) + 3NiCl_2(aq) -> Ni3(PO4)_2(s) + 6KCl(aq)}$$

5. Write balanced net ionic equation for the reaction

$$\ce{2K_3PO_4(aq) + 3NiCl_2(aq) -> Ni3(PO4)_2(s) + 6KCl(aq)}$$

Complete and balance the following neutralization reactions.

HNO$_{3}$(aq) + Ca(OH)$_{2}$ (aq) $\rarr$

Complete the following neutralization reactions. Balance each reaction, and then write the overall ionic and net ionic equation for each. a.

$$\mathrm { HCl } ( a q ) + \mathrm { NaOH } ( a q ) \longrightarrow$$

, b.

$$\mathrm { HNO } _ { 3 } ( a q ) + \mathrm { KOH } ( a q ) \longrightarrow$$

, c.

$$\mathrm { Ca } ( \mathrm { OH } ) _ { 2 } ( a q ) + \mathrm { HNO } _ { 3 } ( a q ) \longrightarrow$$

, d.

$$\operatorname { Mg } ( \mathrm { OH } ) _ { 2 } ( a q ) + \mathrm { HCl } ( a q ) \longrightarrow$$

Chlorine has two stable nuclides, ${ }^{35} \mathrm{Cl}$ and ${ }^{37} \mathrm{Cl}$. In contrast, ${ }^{36} \mathrm{Cl}$ is a radioactive nuclide that decays by beta emission.

What is the product of decay of ${ }^{36} \mathrm{Cl}$ ?

Finish the given chemical equation:

$$\ce{HNO3(aq) +K2SO3(aq)→}$$