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Chapter 14: Problem 2

Differentiate between the terms strength and concentration as they apply to acids and bases. When is HCl strong? Weak? Concentrated? Dilute? Answer the same questions for ammonia. Is the conjugate base of a weak acid a strong base?

Short Answer

Expert verified
The strength of an acid or base refers to its ability to dissociate in water, while concentration describes the amount of acid or base in a solution. HCl is a strong acid and can be concentrated or dilute depending on the moles per liter. Ammonia is a weak base and also can be concentrated or dilute. Generally, the conjugate base of a weak acid is a strong base, as it has a high tendency to react with water and form hydroxide ions, though there are exceptions.

Step by step solution

01

Definition of strength

The strength of an acid or base refers to its ability to dissociate in water, forming ions. A strong acid or base is one that almost completely dissociates into its constituent ions, while a weak acid or base does not dissociate completely, and a significant amount of the molecule remains in its original form.
02

Definition of concentration

Concentration, on the other hand, describes the amount of an acid or base dissolved in a solution. It is typically expressed in moles per liter (M). A concentrated acid or base has a high amount of the substance in the solution, while a dilute acid or base has a lower amount. #Step 2: Describe properties of HCl#
03

HCl strength

Hydrochloric acid (HCl) is a strong acid. This means that it almost completely dissociates in water forming hydrogen ions (H+) and chloride ions (Cl-).
04

HCl concentration

HCl can be concentrated or diluted depending on the amount of HCl dissolved in water. For example, a 12 M HCl solution is considered concentrated, while a 0.1 M solution is considered diluted. #Step 3: Describe properties of ammonia#
05

Ammonia strength

Ammonia (NH3) is a weak base. In water, it reacts partially with water molecules to produce hydroxide ions (OH-) and ammonium ions (NH4+), but a significant amount of ammonia molecules remain undissociated in the solution.
06

Ammonia concentration

Like HCl, ammonia can be concentrated or diluted depending on the amount of NH3 dissolved in water. For example, a 14.8 M ammonia solution is considered concentrated, and a 0.01 M solution is considered diluted. #Step 4: Conjugate base of a weak acid#
07

Relationship between weak acid and its conjugate base

The conjugate base of a weak acid is generally a strong base. This is because a weak acid does not dissociate completely in water, leaving a lot of its conjugate base undissociated. In order for an equilibrium to be established, the conjugate base must have a strong tendency to react with water and form hydroxide ions (OH-). However, this is not universally true as there are exceptions where the conjugate base of a weak acid is also weak.

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Most popular questions from this chapter

The equilibrium constant \(K_{\mathrm{a}}\) for the reaction \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q)+\mathrm{H}_{2} \mathrm{O}(l)=\) \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}(\mathrm{OH})^{2+}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)\) is \(6.0 \times 10^{-3}\). a. Calculate the \(\mathrm{pH}\) of a \(0.10 \mathrm{M}\) solution of \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\). b. Will a \(1.0 M\) solution of iron(II) nitrate have a higher or lower \(\mathrm{pH}\) than a \(1.0 \mathrm{M}\) solution of iron(III) nitrate? Explain.

A typical vitamin C tablet (containing pure ascorbic acid, \(\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{6}\) ) weighs 500 . mg. One vitamin C tablet is dissolved in enough water to make \(200.0 \mathrm{~mL}\) of solution. Calculate the \(\mathrm{pH}\) of this solution. Ascorbic acid is a diprotic acid.

Using your results from Exercise 129, place the species in each of the following groups in order of increasing base strength. a. \(\mathrm{OH}^{-}, \mathrm{SH}^{-}, \mathrm{SeH}^{-}\) b. \(\mathrm{NH}_{3}, \mathrm{PH}_{3}\) c. \(\mathrm{NH}_{3}, \mathrm{HONH}_{2}\)

Rank the following \(0.10 \mathrm{M}\) solutions in order of increasing \(\mathrm{pH}\). a. HI, HF, NaF, NaI b. \(\mathrm{NH}_{4} \mathrm{Br}, \mathrm{HBr}, \mathrm{KBr}, \mathrm{NH}_{3}\) c. \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{NO}_{3}, \mathrm{NaNO}_{3}, \mathrm{NaOH}, \mathrm{HOC}_{6} \mathrm{H}_{5}, \mathrm{KOC}_{6} \mathrm{H}_{5}, \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\), \(\mathrm{HNO}_{3}\)

A codeine-containing cough syrup lists codeine sulfate as a major ingredient instead of codeine. The Merck Index gives \(\mathrm{C}_{36} \mathrm{H}_{44} \mathrm{~N}_{2} \mathrm{O}_{10} \mathrm{~S}\) as the formula for codeine sulfate. Describe the composition of codeine sulfate. (See Exercise 143.) Why is codeine sulfate used instead of codeine?
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