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Chapter 4: Q4.49P (page 180)

Limestone (calcium carbonate) is insoluble in water but dissolves when a hydrochloric acid solution is added. Write balanced total ionic and net ionic equations, showing hydrochloric acid as it actually exists in water and the reaction as a proton-transfer process.

Short Answer

Expert verified

A carbonate ion is a base and hydrochloric acid is an acid. When both react, they form H2CO3 which further decomposes into CO2 gas and water as the final products.

Step by step solution

01

Determine different types of equations to represent aqueous ionic reactions

The molecular equation reveals the least about the species in solution and is actually somewhat misleading because it shows all the reactants and products as if they were intact undissociated compounds.

The total ionic equation is a much more accurate representation of the reaction because it shows all the soluble ionic substances dissociated into ions.

The net ionic equation is the most useful because it omits the spectator ions and shows the actual chemical change taking place.

02

Write the net ionic equation of the reaction between calcium carbonate and hydrochloric acid

Balanced molecular reaction:

CaCO3(s)+2HCl(aq)鈫�CaCl2(aq)+H2CO3(aq)

Total ionic equation:

CaCO3(s)+2H+(aq)+2Cl-(aq)鈫�Ca2+(aq)+2Cl-(aq)+H2O(l)+CO2(g)

Net ionic equation:

CaCO3(s)+2H+(aq)鈫�Ca2+(aq)+H2O(l)+CO2(g)

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Most popular questions from this chapter

An unknown amount of acid can often be determined by adding an excess of base and then 鈥渂ack-titrating鈥� the excess. A 0.3471-g sample of a mixture of oxalic acid, which has two ionizable protons, and benzoic acid, which has one, is treated with 100.0 mL of 0.1000 M NaOH. The excess NaOH is titrated with 20.00 mL of 0.2000 M HCl. Find the mass % of benzoic acid.

Give the oxidation number of carbon in the following:

(a)CF2Cl2(b)Na2C2O4(c)HCO3-(d)C2H6

If 26.25 mL of a standard 0.1850 M NaOH solution is required to neutralize 25.00 mL of H2SO4, what is the molarity of the acid solution?

A reaction cyclefor an element is a series of reactions beginning and ending with that element. In the following copper reaction cycle, copper has either a 0 or a _2 oxidation state. Write balanced molecular and net ionic equations for each step in the cycle.

(1) Copper metal reacts with aqueous bromine to produce a green-blue solution.

(2) Adding aqueous sodium hydroxide forms a blue precipitate.

(3) The precipitate is heated and turns black (water is released).

(4) The black solid dissolves in nitric acid to give a blue solution.

(5) Adding aqueous sodium phosphate forms a green precipitate.

(6) The precipitate forms a blue solution in sulfuric acid.

(7) Copper metal is recovered from the blue solution when zinc metal is added.

Question: How many moles ofions are present in the following aqueous solutions?

(a) 1.4 mL of 0.75 M hydrobromic acid

(b) 2.47 mL of 1.98 M hydriodic acid

(c) 395 mL of 0.270 M nitric acid
See all solutions

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