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Math

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PROBLEM

Identify each of the following as acidic, basic, or neutral:
1. a solution where the H3O+\mathrm{H}_{3} \mathrm{O}^{+}concentration is greater than the OH\mathrm{OH}^{-}concentration
[ Select ]
2. a solution that is 0.25 M NaOH
[ Select ]
3. a solution that is 1.0 M HCl [ Select ]
4. a solution that has a pH of 10 [Select]
5. a solution of NaCl [ Select]

STEP 1

1. The nature of a solution (acidic, basic, or neutral) can be determined by comparing the concentrations of H3O+\mathrm{H}_{3}\mathrm{O}^{+} and OH\mathrm{OH}^{-}.
2. The pH scale is used to determine the acidity or basicity of a solution.
3. Strong acids and bases completely dissociate in water.
4. NaCl is a neutral salt.

STEP 2

1. Analyze the relationship between H3O+\mathrm{H}_{3}\mathrm{O}^{+} and OH\mathrm{OH}^{-}.
2. Determine the nature of the solution based on the concentration of NaOH.
3. Determine the nature of the solution based on the concentration of HCl.
4. Determine the nature of the solution based on its pH value.
5. Determine the nature of a NaCl solution.

STEP 3

If the H3O+\mathrm{H}_{3}\mathrm{O}^{+} concentration is greater than the OH\mathrm{OH}^{-} concentration, the solution is acidic.

STEP 4

NaOH is a strong base. A 0.25 M NaOH solution is basic because it dissociates completely to produce OH\mathrm{OH}^{-} ions.

STEP 5

HCl is a strong acid. A 1.0 M HCl solution is acidic because it dissociates completely to produce H3O+\mathrm{H}_{3}\mathrm{O}^{+} ions.

STEP 6

A solution with a pH of 10 is basic because a pH greater than 7 indicates a basic solution.

SOLUTION

NaCl is a neutral salt formed from a strong acid (HCl) and a strong base (NaOH). A solution of NaCl is neutral.
The nature of each solution is as follows:
1. Acidic
2. Basic
3. Acidic
4. Basic
5. Neutral

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