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Ch.4 - Reactions in Aqueous Solution
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.4 - Reactions in Aqueous SolutionProblem 88b
Chapter 4, Problem 88b

A solution is made by mixing 1.5 g of LiOH and 23.5 mL of 1.000 M HNO3. (b) Calculate the concentration of each ion remaining in solution.

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Determine the moles of LiOH using its molar mass: \( \text{moles of LiOH} = \frac{1.5 \text{ g}}{\text{molar mass of LiOH}} \).
Calculate the moles of HNO3 using its concentration and volume: \( \text{moles of HNO3} = 1.000 \text{ M} \times 0.0235 \text{ L} \).
Write the balanced chemical equation for the reaction: \( \text{LiOH} + \text{HNO}_3 \rightarrow \text{LiNO}_3 + \text{H}_2\text{O} \).
Determine the limiting reactant by comparing the moles of LiOH and HNO3.
Calculate the moles of Li+ remaining in solution, considering the stoichiometry of the reaction and the limiting reactant.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this case, understanding the stoichiometric ratios between LiOH and HNO3 is essential to find out how much Li+ remains after the reaction.
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Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is crucial for calculating the concentration of ions in a solution. In this question, the molarity of HNO3 is given, which will help determine how many moles of HNO3 are present and how they react with LiOH.
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Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this scenario, HNO3 (an acid) reacts with LiOH (a base) to form water and LiNO3. Understanding this concept is vital for determining the extent of the reaction and calculating the remaining concentration of Li+ in the solution.
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Related Practice
Textbook Question

A 0.5895-g sample of impure magnesium hydroxide is dissolved in 100.0 mL of 0.2050 M HCl solution. The excess acid then needs 19.85 mL of 0.1020 M NaOH for neutralization. Calculate the percentage by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the HCl solution.

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Textbook Question

A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO4. (a) Write the balanced chemical equation for the reaction that occurs.

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Textbook Question

A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid–base indicator is added, and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 17.0 mL of the hydrochloric acid solution has been added. (b) What is the identity of the alkali metal cation: Li+, Na+, K+, Rb+, or Cs+?

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Textbook Question

A solution is made by mixing 1.5 g of Sr(OH)2 and 23.5 mL of 1.000 M HNO3. (c) Is the resulting solution acidic or basic?

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Textbook Question

A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO4. (b) What precipitate forms?

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Textbook Question

A 1.248-g sample of limestone rock is pulverized and then treated with 30.00 mL of 1.035 M HCl solution. The excess acid then requires 11.56 mL of 1.010 M NaOH for neutralization. Calculate the percentage by mass of calcium carbonate in the rock, assuming that it is the only substance reacting with the HCl solution.

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