How many milliliters of 2.00 M HCl must be added to neutralize the following solutions? (a) A mixture of 0.160 M HNO3 (100.0 mL) and 0.100 M KOH (400.0 mL)

Verified step by step guidance

1. Calculate the moles of HNO3 using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).
2. Calculate the moles of KOH using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).
3. Determine the net moles of acid or base by subtracting the moles of KOH from the moles of HNO3.
4. Use the net moles of acid or base to find the volume of 2.00 M HCl needed for neutralization using the formula: \( \text{volume} = \frac{\text{moles}}{\text{concentration}} \).
5. Convert the volume from liters to milliliters by multiplying by 1000.

Key Concepts

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this context, hydrochloric acid (HCl) will react with potassium hydroxide (KOH) to form water and potassium chloride (KCl). Understanding the stoichiometry of this reaction is essential for calculating the volumes of acid and base needed for complete neutralization.

Molarity (M)

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. In this question, the molarity of HCl, HNO3, and KOH is given, which allows for the calculation of the number of moles present in each solution. This is crucial for determining how much HCl is required to neutralize the given amounts of HNO3 and KOH.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. In this scenario, it is necessary to use stoichiometric ratios derived from the balanced equation of the neutralization reaction to find the exact volume of HCl needed to neutralize the acids and bases present in the mixtures. This ensures that the correct amounts are used for complete reaction.