Question

The pH of a basic solution is 9.77. What is [OH⁻]?

Answer 1

The  [OH⁻] of the solution is 5.37×10⁵ M.

What is pOH?

This is the negative logarithm to base 10 of hydroxy ion [OH⁻] concentration.

To calculate the hydroxy ion [OH⁻] concentration we use the formula below.

Note:

• pH+pOH = 14

• pOH = 14-pH
• pOH = 14-9.77
• pOH = 4.27

Formula:

• [OH⁻] = 1/$10^{pOH}$................. Equation 1

Given:

• pOH = 4.27

Substitute the value into equation 1

• [OH⁻] = 1/$10^{4.27}$
• [OH⁻]  = 5.37×10⁵

Hence, The [OH⁻] of the solution is 5.37×10⁵ M.

Learn more about hydroxy ion concentration here: brainly.com/question/17090407

Answer 2

The concentration of the hydroxide ion [OH¯] in the solution is 5.89×10¯⁵ M

How to determine the pOH

From the question given above, the following data were obtained:

• pH = 9.77

• pOH =?

pH + pOH = 14

9.77 + pOH = 14

Collect like terms

pOH = 14 – 9.77

pOH = 4.23

How to determine [OH¯]

• pOH = 4.23

• Concentration of Hydroxide ion [OH¯] =?

pOH = –Log [OH¯]

4.23 = –Log [OH¯]

Multiply through by –1

–4.23 = Log [OH¯]

Take the anti-log of –4.23

[OH¯] = anti-log (–4.23)

[OH¯] = 5.89×10¯⁵ M

Learn more about pH:

brainly.com/question/3709867