A solution of nitric acid of specific gravity 1.46 contains 60% nitric acid. What weight of this solution is theoretically required to dissolve 5 g of cupric oxide?

Explanation

To solve the problem step by step, we will first write the balanced chemical equation for the reaction between cupric oxide (CuO) and nitric acid (HNO3). Then we will determine how much nitric acid is needed to dissolve 5 grams of cupric oxide. Finally, we will calculate the weight of the nitric acid solution required to provide that amount of nitric acid.

### Step 1: Write the balanced chemical equation
The reaction between cupric oxide and nitric acid can be written as:
\[ \text{CuO} + 2 \text{HNO}_3 \rightarrow \text{Cu(NO}_3)_2 + \text{H}_2\text{O} \]

### Step 2: Determine moles of CuO
First, we need to calculate the molar mass of CuO:
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