We’re being asked to determine the limiting reactant for the reaction that occurs when 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.
For this problem, we need to do the following steps:
Step 1: Determine the products of the reaction.
Step 2: Write and balance a chemical equation for the given reaction.
Step 3: Determine the limiting reactant
Recall that the limiting reactant, is the reactant that forms the less amount of product. This is because once the limiting reactant is all used up, the reaction can no longer proceed and make more products.
Step 1: Since KOH and NiSO4 are ionic compounds, they form ions when dissociating in water. The dissociation of the two compounds is as follows:
The hydroxide ion, OH–, has a charge of –1. Potassium, K is from Group 1 so it has a charge of +1:
KOH(aq) ⇌ K+(aq) + OH–(aq)
The sulfate ion, SO42–, has a charge of –2. Nickel, Ni then has a charge of +2:
NiSO4 (aq) ⇌ Ni2+(aq) + SO42–(aq)
**Recall that for ionic compounds with the same numerical charge, the subscript is not written
A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.
What is the limiting reactant?
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What scientific concept do you need to know in order to solve this problem?
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Based on our data, we think this problem is relevant for Professor Roy's class at GMU.