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Hatshy [7]
3 years ago
10

What is the name for the point at which the indicator changes color in a titration? turning point end point indicator point colo

r point NextReset
Chemistry
2 answers:
Sedaia [141]3 years ago
8 0
It says on google
<span>An acid-base indicator (e.g., phenolphthalein) changes color depending on the pH. Redox indicators are also frequently used. A drop of indicator solution is added to the titration at the start; when the color changes the endpoint has been reached, this is an approximation of the equivalence point.</span>
Aloiza [94]3 years ago
8 0

Answer:

End point

Explanation:

Titration is a method of quantitative analysis which is employed to determine the concentration of unknown solutions.

Here a titrant of known concentration is added to a given volume of an analyte solution along with a suitable indicator. The titrant is added gradually until a color change in the analyte is observed. This point is known as the end point.

The end point is usually approximated as the equivalence point wherein the moles of titrant consumed equals the moles of analyte present.

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What is the pH of a solution that is 0.40 M NaBrO and 0.50 M HBrO (hypobromous acid) (Ka for HBrO = 2.3 x 10^-9)
Pie

Answer

pH=8.5414

Procedure

The Henderson–Hasselbalch equation relates the pH of a chemical solution of a weak acid to the numerical value of the acid dissociation constant, Kₐ. In this equation, [HA] and [A⁻] refer to the equilibrium concentrations of the conjugate acid-base pair used to create the buffer solution.

pH = pKa + log₁₀ ([A⁻] / [HA])

Where

pH = acidity of a buffer solution

pKa = negative logarithm of Ka

Ka =acid disassociation constant

[HA]= concentration of an acid

[A⁻]= concentration of conjugate base

First, calculate the pKa

pKa=-log₁₀(Ka)= 8.6383

Then use the equation to get the pH (in this case the acid is HBrO)

pH=8.6383+\log_{10}(\frac{0.40\text{ M}}{0.50\text{ M}})=8.5414

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