Arrange the following 0.5 M aqueous solutions in order of increasing pH NaOH, HBr, NaCH3 CO2, KB

step 1 In this question, we have to take 0 .5 molar of each of the following compounds in a solution. A

Arrange the following 0.5 M aqueous solutions in order of...

Arrange the following $0.5 \mathrm{M}$ aqueous solutions in order of increasing $\mathrm{pH}$ $\mathrm{NaOH}, \mathrm{HBr}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}, \mathrm{KBr}, \mathrm{NH}_{4} \mathrm{Br}$ a. $\mathrm{HBr}, \mathrm{NH}_{4} \mathrm{Br}, \mathrm{KBr}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}, \mathrm{NaOH}$ b. $\mathrm{NaOH}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}, \mathrm{KBr}, \mathrm{NH}_{4} \mathrm{Br}, \mathrm{HBr}$ c. $\mathrm{NaOH}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}, \mathrm{NH}_{4} \mathrm{Br}, \mathrm{KBr}, \mathrm{HBr}$ d. $\mathrm{HBr}, \mathrm{KBr}, \mathrm{NH}_{4} \mathrm{Br}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}, \mathrm{NaOH}$

Arrange the following $0.5 \mathrm{M}$ aqueous solutions in order of increasing $\mathrm{pH}$
$\mathrm{NaOH}, \mathrm{HBr}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}, \mathrm{KBr}, \mathrm{NH}_{4} \mathrm{Br}$
a. $\mathrm{HBr}, \mathrm{NH}_{4} \mathrm{Br}, \mathrm{KBr}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}, \mathrm{NaOH}$
b. $\mathrm{NaOH}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}, \mathrm{KBr}, \mathrm{NH}_{4} \mathrm{Br}, \mathrm{HBr}$
c. $\mathrm{NaOH}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}, \mathrm{NH}_{4} \mathrm{Br}, \mathrm{KBr}, \mathrm{HBr}$
d. $\mathrm{HBr}, \mathrm{KBr}, \mathrm{NH}_{4} \mathrm{Br}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}, \mathrm{NaOH}$

Key Concepts

Weak Base Salts

Weak base salts, derived from a weak base combined with a strong acid, can also undergo hydrolysis in water, but they typically produce an acidic solution. The extent of the acidity depends on the strength of the weak base, and such salts result in pH values lower than neutral solutions.

Salt Hydrolysis

Salt hydrolysis refers to the reaction of salt ions with water, which can affect the pH of the solution. Salts derived from a strong acid and a strong base tend to be neutral, while those from a weak acid with a strong base form basic solutions, and salts from a strong acid with a weak base form acidic solutions.

Weak Acid Salts

Weak acid salts, such as those whose anions come from weak acids, are capable of undergoing hydrolysis in water. This reaction can make the resulting solution basic, though not as strongly basic as a strong base solution, influencing the pH order of different solutions.

Strong Acids

Strong acids completely dissociate in water, releasing a high concentration of hydrogen ions. This characteristic leads to very low pH values in their aqueous solutions, which is an important factor when arranging solutions by increasing pH.

pH is a measure of the acidity or basicity of an aqueous solution. It is defined as the negative logarithm of the hydrogen ion concentration. Understanding pH is fundamental when comparing solutions, as lower pH values indicate acidic solutions, while higher pH values indicate basic solutions.

Strong Bases

Strong bases fully dissociate in water, producing a high concentration of hydroxide ions. Their complete ionization results in very high pH values, a key concept when ordering solutions from acidic to basic.

Transcript

Please give Ace some feedback