QuestionIdentify each of the following as acidic, basic, or neutral:
1. a solution where the $\mathrm{H}_{3} \mathrm{O}^{+}$ concentration is greater than the $\mathrm{OH}^{-}$ 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]

Studdy Solution

STEP 1

1. The nature of a solution (acidic, basic, or neutral) can be determined by comparing the concentrations of $\mathrm{H}_{3}\mathrm{O}^{+}$ and $\mathrm{OH}^{-}$ .
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 $\mathrm{H}_{3}\mathrm{O}^{+}$ and $\mathrm{OH}^{-}$ .
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 $\mathrm{H}_{3}\mathrm{O}^{+}$ concentration is greater than the $\mathrm{OH}^{-}$ 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 $\mathrm{OH}^{-}$ ions.

STEP 5

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

STEP 6

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

STEP 7

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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Studdy Solution

STEP 1

STEP 2

STEP 3

If the $\mathrm{H}_{3}\mathrm{O}^{+}$ concentration is greater than the $\mathrm{OH}^{-}$ 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 $\mathrm{OH}^{-}$ ions.

STEP 5

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

STEP 6

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

STEP 7

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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Studdy Solution

STEP 1

STEP 2

STEP 3

If the H3O+\mathrm{H}_{3}\mathrm{O}^{+}H3​O+ concentration is greater than the OH−\mathrm{OH}^{-}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}^{-}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}^{+}H3​O+ ions.

STEP 6

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

STEP 7

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. Acidic2. Basic3. Acidic4. Basic5. Neutral

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

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

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

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