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A 1. 2×10−5mol sample of ca(oh)2 is dissolved in water to make up 250. 0 ml of solution. What is the ph of the solution at 25. 0∘c? round your answer to the hundredths place

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mahima6824soni

1. 2×10−5molA 1. 2×10−5mol sample of ca(oh)2 is dissolved in water. The pH o steh sample is

What is pH?

pH is potential hydrogen. It is the measurement of the acidity and basicity of any solution.

The ca(oh)2 sample is 1. 2×10−5 mol.

To calculate the pH, the formula is pH = -log[H3O+]

First, calculate the molarity of ca(oh)2 is 4.8 x 10-5M

[OH-] = 9.6 x 10-5M

[OH-][H3O+] = kw (1.0 x 10-14)

[H3O+] =  kw /  [OH-]    

[H3O+] = 1.0 x 10-14 / 9.6 x 10-5

[H3O+]= 1.04 x 10-10M

pH= -log[1.04 x 10-10M]

pH= 9.98

Thus, the pH is 9.98

Learn more about pH

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