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If a 50.00 mL of 0.0155 M HI(aq) is mixed with 75.00 mL of 0.0106 M KOH(aq), what is the pH of the final solution

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okpalawalter8

If a 50.00 mL of 0.0155 M HI(aq) is mixed with 75.00 mL of 0.0106 M KOH(aq), the pH of the final solution  is mathematically given as

pH=13.16

What is the pH of the final solution?

Generally, the equation for the Chemical reaction   is mathematically given as

2HI+Ba(OH_2)--->BaI2+2H2O

Therefore

pOH=-log{OH}

pOH=-log(6.52)

pOH=0.8142

In conclusion, for the pH

pH+pOH=14

pH=14-0.8142

pH=13.16

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