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Chapter 7: Problem 57

Which addition would not change the \(\mathrm{pH}\) of \(10 \mathrm{ml}\) of dilute hydrochloric acid? (1) \(20 \mathrm{ml}\) of the same hydrochloric acid (2) \(5 \mathrm{ml}\) of pure water (3) \(20 \mathrm{ml}\) of purc water (4) \(10 \mathrm{ml}\) of concentrated hydrochloric acid

Short Answer

Expert verified
Adding 5 ml of pure water (Option 2) would not notably change the \(\rm{pH}\).

Step by step solution

01

Analyze the given solutions

Evaluate each option and its potential impact on the \(\rm{pH}\) of the dilute hydrochloric acid.
02

Evaluate Option 1

Adding more of the same hydrochloric acid (20 ml) would increase the concentration of hydrogen ions \(H^+\), thus decreasing the \(\rm{pH}\).
03

Evaluate Option 2

Adding 5 ml of pure water would slightly dilute the solution, potentially increasing the \(\rm{pH}\) a little, but not significantly.
04

Evaluate Option 3

Adding 20 ml of pure water would significantly dilute the solution, raising its \(\rm{pH}\) noticeably.
05

Evaluate Option 4

Adding 10 ml of concentrated hydrochloric acid would increase the concentration of hydrogen ions \(H^+\) in the solution, decreasing the \(\rm{pH}\).
06

Determine the correct answer

The correct choice brings almost no change in the \(\rm{pH}\) level. Among the options, adding 5 ml of pure water is the one that would cause the least change in the \(\rm{pH}\).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

pH change
Understanding \(\rm{pH}\) change is crucial in acid-base chemistry. \(\rm{pH}\) is a measure of the hydrogen ion concentration in a solution. The \(\rm{pH}\) scale ranges from 0 to 14. Lower values mean a solution is more acidic, while higher values mean it is more basic. Pure water has a neutral \(\rm{pH}\) of 7.

The \(\rm{pH}\) changes when substances that alter hydrogen ion concentration are added. For instance, adding hydrochloric acid, which releases hydrogen ions, will lower the \(\rm{pH}\). Conversely, adding a basic substance will increase the \(\rm{pH}\) by reducing the hydrogen ion concentration. When evaluating the effects of substances on \(\rm{pH}\), consider their capability to donate or accept hydrogen ions.
dilution effect
Dilution occurs when more solvent, usually water, is added to a solution. This can change the concentration of solutes, impacting the solution's \(\rm{pH}\).

When you dilute an acid like hydrochloric acid, the concentration of hydrogen ions \((\rm{H}^+)\) decreases. This causes the \(\rm{pH}\) to rise, making the solution less acidic. The degree of \(\rm{pH}\) change depends on how much solvent you add. Small amounts might only slightly affect the \(\rm{pH}\), while larger quantities can significantly increase it.
hydrochloric acid
Hydrochloric acid (\rm{HCl}) is a strong acid commonly found in laboratory and industrial settings. It fully dissociates in water, meaning it releases all of its hydrogen ions \((\rm{H}^+)\). This leads to a very low \(\rm{pH}\) and strong acidity.

When you add hydrochloric acid to a solution, it significantly increases the hydrogen ion concentration, lowering the \(\rm{pH}\). Knowing this helps in analyzing how different volumes or concentrations of \rm{HCl} impact the \(\rm{pH}\) of a solution. For instance, adding more \rm{HCl} will further reduce the \(\rm{pH}\), while dilution with water will reduce its acidity.
hydrogen ion concentration
Hydrogen ion concentration \((\rm{H}^+)\) is key in determining the \(\rm{pH}\) of a solution. The relationship is given by the equation: \[\rm{pH} = -\text{log}[\rm{H}^+]\]

In this equation, \([\rm{H}^+]\) represents the molar concentration of hydrogen ions. A high \([\rm{H}^+]\) means a low \(\rm{pH}\), indicating an acidic solution. Conversely, a low \([\rm{H}^+]\) means a high \(\rm{pH}\) and a basic solution.

Understanding these principles helps in predicting how additions of certain substances, like hydrochloric acid or water, can alter the \(\rm{pH}\) by affecting the \([\rm{H}^+]\).

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Most popular questions from this chapter

Which of the following statements is falsc? (1) Hydrolysis of the salt of strong acid and weak base is called cationic hydrolysis (2) Hydrolysis of the salt of weak acid and strong base is known as anionic hydrolysis (3) Aqueous solution of aluminium chloride is acidic due to hydrolysis of \(\mathrm{Al}^{3}\) ion (4) Aqueous solution of sodium carbonate is basic due to hydrolysis of \(\mathrm{Na}\) ion

The equilibrium constant for the reaction \(\mathrm{Br}_{2} \rightleftharpoons\) \(2 \mathrm{Br}\) at \(500 \mathrm{~K}\) and \(700 \mathrm{~K}\) are \(1 \times 10^{\circ}\) and \(1 \times 10^{5}\), respectively. The reaction is (1) endothermic (2) exothermic (3) fast (4) slow

\(A\) mixturc of a weak acid (say acctic acid) and its salts with a strong basc (say sodium acetate) acts as a buffcr solution. Which other pair has similar properties? (1) IICl and \(\mathrm{NaCl}\) (2) \(\mathrm{NaOII}\) and \(\mathrm{NaNO}_{3}\) (3) KOII and KCl (4) \(\mathrm{NII}_{4} \mathrm{OII}\) and \(\mathrm{NII}_{4} \mathrm{Cl}\)

To \(100 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{AgNO}_{3}\) solution, solid \(\mathrm{K}_{2} \mathrm{SO}_{4}\) is added. The concentration of \(\mathrm{K}_{2} \mathrm{SO}_{4}\) that shows the precipitation is \(\left(K_{s p}\right.\) for \(\left.\mathrm{A}_{\mathrm{g}_{2}} \mathrm{SO}_{4}=6.4 \times 10^{-5} \mathrm{M}\right)\) (1) \(0.1 \mathrm{M}\) (2) \(6.4 \times 10^{-3} \mathrm{M}\) (3) \(6.4 \times 10^{-7} \mathrm{M}\) (4) \(6.4 \times 10^{-5} \mathrm{M}\)

The correct statement is (1) \(\mathrm{NII}_{4} \mathrm{Cl}\) gives an alkalinc solution in water (2) \(\mathrm{CII}_{3}\) COONa gives an acidic solution in water (3) \(\mathrm{CII}_{3} \mathrm{COOII}\) is a weak acid (4) \(\mathrm{NII}_{4} \mathrm{OII}\) is a strong base
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