Question

what volume of a 0.138 m potassium hydroxide solution is required to neutralize 26.0 ml of a 0.205 m nitric acid solution?

Answer 1

A neutralization titration is a chemical response this is used to decide the composition of an answer and what kind of acid or base is in it. This is a way of volumetric analysis and the formula is ($M1V1 = M2V2$).

Utilize the titration method of $M1V1 = M2V2$ in view that we're given the concentrations of every compound and the quantity of $KOH$. Let: M1 = 0.138M, V1 = x, M2 = 0.205M, V2 = 26.0 ML.

• M1 = initial mass
• V1= initial volume
• M2 = final mass
• V2= final volume

• $(M1V1 = M2V2)$
• (0.138)(V1) = (0.205)x(26.0)
• V2=(0.205)x(26.0)\ 0.138
• V2 = 47.10 M/L
• The final value of Volume needed for neutralization of nitric acid solution is  V2 = 47.10 M/L

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