Formulae and Equation Writing: Practice Questions

What is the chemical formula for the ionic compound sodium phosphate?

Which ionic equation correctly represents the reaction between aqueous barium nitrate and aqueous potassium sulfate?

Phosphine gas, \(\text{PH}_3\), reacts with aqueous copper(II) sulfate to form solid copper(II) phosphide, \(\text{Cu}_3\text{P}_2\), and dilute sulfuric acid according to the following unbalanced chemical equation:
\(p\text{PH}_3\text{(g)} + q\text{CuSO}_4\text{(aq)} \rightarrow r\text{Cu}_3\text{P}_2\text{(s)} + s\text{H}_2\text{SO}_4\text{(aq)}\)

What is the value of the ratio \(\frac{p + s}{q + r}\) when the equation is balanced using the lowest whole number integers?

What is the correct chemical formula for the ionic compound formed between aluminium ions and sulfate ions?

Which ionic equation, including state symbols, correctly represents the reaction between excess dilute nitric acid and solid copper(II) carbonate?

State the chemical formula of the ionic compound formed between aluminium ions, \( \text{Al}^{3+} \), and sulfate ions, \( \text{SO}_4^{2-} \).

Construct the balanced chemical equation, including state symbols, for the reaction between solid calcium carbonate and dilute hydrochloric acid.

When solid lead(II) nitrate is heated, it decomposes thermally into solid lead(II) oxide, brown nitrogen dioxide gas, and oxygen gas.

(a) Construct the balanced chemical equation, including state symbols, for the thermal decomposition of solid lead(II) nitrate, ext{Pb(NO}_3)_2 ext{.}
(b) Construct the balanced ionic equation, including state symbols, for the reaction between aqueous sodium hydroxide and aqueous iron(III) chloride.

When solid magnesium carbonate reacts with dilute hydrochloric acid, magnesium chloride solution, water, and carbon dioxide gas are produced.

(a) Write the balanced chemical equation, including state symbols, for this reaction.
(b) Write the ionic equation, including state symbols, for this reaction.

A student investigates several chemical reactions in the laboratory involving various inorganic compounds.

(a) State the chemical formula for iron(III) sulfate.
(b) Solid ammonium sulfate, \((\text{NH}_4)_2\text{SO}_4\), is warmed with aqueous sodium hydroxide, \(\text{NaOH}\). The products formed are aqueous sodium sulfate, water, and ammonia gas. Write the full balanced chemical equation, including state symbols, for this reaction.
(c) Write the balanced ionic equation, including state symbols, for the reaction occurring in part (b).
(d) In another experiment, aqueous lead(II) nitrate, \(\text{Pb(NO}_3)_2\), is mixed with aqueous potassium iodide, \(\text{KI}\), forming a bright yellow precipitate of lead(II) iodide and aqueous potassium nitrate.
(i) Write the full balanced chemical equation, including state symbols, for this precipitation reaction.
(ii) Write the balanced ionic equation, including state symbols, for this precipitation reaction, and state the spectator ions present.