Question

now lets look at another equation: co₃⁻²(aq) + 2h⁺(aq) → h₂o(l) + co₂(g) take a moment to consider how many hydrogen ions (h⁺) will be necessary to completely react with the following amounts of carbonate ion (co₃⁻) and then enter your responses below: five carbonate ions 10 h+ ions 1,500 carbonate ions 3000 h+ ions 2 x 10¹⁵ carbonate ions h+ ions 6.022 x 10²³ carbonate ions h+ ions three moles of carbonate ions 6 moles of h+ ions

Explanation:

Step1: Analyze the stoichiometry of the reaction

From the balanced equation \(CO_{3}^{-2}(aq)+2H^{+}(aq)\to H_{2}O(l) + CO_{2}(g)\), the mole ratio of \(CO_{3}^{-2}\) to \(H^{+}\) is \(1:2\).

Step2: Calculate for \(2\times10^{15}\) carbonate ions

Since the ratio is \(1:2\), the number of \(H^{+}\) ions \(=2\times(2\times 10^{15})=4\times10^{15}\)

Step3: Calculate for \(6.022\times10^{23}\) carbonate ions

Using the \(1:2\) ratio, the number of \(H^{+}\) ions \(=2\times(6.022\times 10^{23}) = 1.2044\times10^{24}\)

Answer:

For \(2\times10^{15}\) carbonate ions: \(4\times10^{15}\) \(H^{+}\) ions
For \(6.022\times10^{23}\) carbonate ions: \(1.2044\times10^{24}\) \(H^{+}\) ions