Q: What is the pH of 3.5 x 10 -4 M solution of KOH?

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Molarity of hydrogen solution equals 2.3 X 10^-4 -log(2.3 X 10^-4) = 3.6 pH

Is always basic.

2

- log(2.3 X 10 -12 ) = 11.6 pH -----------------very little H + concentration in this solution.

-log(9.40 X 10^-4) = 3 pH

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The pH of a 1.0x10^-4 M solution of KOH is approximately 10.4. This is because KOH is a strong base that dissociates completely in water to produce hydroxide ions, which results in a basic solution.

The pH of a 1 x 10^-5 M KOH solution would be approximately 9. For a strong base like KOH, the pH can be calculated by taking the negative logarithm of the concentration of hydroxide ions.

The pH of a 10^-5 M KOH solution would be around 9. For a given concentration of a strong base like KOH, the pH can be calculated using the formula pH = 14 - pOH. Given that pOH = -log[OH-] and [OH-] = 10^-5 M in this case, pOH = 5. Therefore, pH = 14 - 5 = 9.

The pH of a 0.0670 M KOH solution can be calculated using the formula pH = 14 - pOH. Since KOH dissociates completely in water to produce OH- ions, the pOH can be found by taking the negative logarithm of the hydroxide ion concentration (0.0670 M in this case). Then, pH = 14 - pOH, allowing you to determine the solution's pH.

The pH of water increase.

The pH of a 0.04 M KOH solution can be calculated by using the formula pH = 14 - pOH. In this case, the pOH is equal to -log(KOH concentration), so pOH = -log(0.04) = 1.4. Therefore, pH = 14 - 1.4 = 12.6.

No, KOH (potassium hydroxide) is a strong base, making it alkaline in nature. It will increase the pH of a solution when added.

The pH electrode is dipped in saturated KOH solution to create a stable reference potential. The presence of potassium ions in the solution helps maintain a stable potential between the reference electrode and the sensing electrode, enabling accurate pH measurements.

The pH meter is kept in saturated KOH solution to maintain the electrode's sensitivity and responsiveness by keeping the reference electrode hydrated and stable. The KOH solution helps to maintain a stable potential at the reference electrode, ensuring accurate pH measurements.

A pH 7 solution is neutral, indicating a balance of acidic and basic components, while a pH 10 solution is basic, meaning it has a higher concentration of hydroxide ions. The pH scale is logarithmic, so a pH 10 solution is 1000 times more basic than a pH 7 solution.

To find the H ion concentration in a KOH solution, first determine the hydroxide ion (OH-) concentration. Since KOH is a strong base, it fully dissociates in water. Therefore, the OH- concentration is equal to the KOH concentration, which is 4.8x10^-2 M. The H ion concentration can be calculated using the equation Kw = [H+][OH-], where Kw is the ion product of water (1.0x10^-14 at 25°C). From there, you can determine the H ion concentration by dividing Kw by the OH- concentration.

The pH of a solution is defined as -log10[H+]. Thus a solution with a hydrogen ion concentration of 10-5M has a pH of 5. [H+] = 10-5 pH = -log[H+] pH = - log [10-5] pH = 5