## What is the reaction between KHP and NaOH?

reaction is called a neutralization reaction because two caustic compounds, KHP, a mild acid, and NaOH, a strong base, are replaced by water and a weaker base.

## How do you standardize NaOH with KHP?

To Standardize: Weigh ~0.8 g of dried KHP (MW = 204.23 g/mol) into an Erlenmeyer flask and dissolve in 50-75 mL of distilled water. Record the amount of KHP and water used. Add 4 drops of indicator into the flask and titrate to the first permanent appearance of pink.

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## How do you calculate the molar amount of Khp used to neutralize the NaOH solution?

Calculate the molar amount of KHP used to neutralize the NaOH solution Number of moles of KHP = 0.5056 g/ 204.23 g/mol = 2.476 x 10 -3 moles 2.

## Why do we use NaOH in titration?

During the course of the titration, the titrant (NaOH) is added slowly to the unknown solution. After the equivalence point, there will be an excess of NaOH and the solution will be basic. An acid-base indicator can be used to help identify when the change from acidic to basic occurs.

## How do you standardize NaOH?

To standardize NaOH, start by pipetting 10.0 ml of 0.1 N hydrochloric acid (HC1) into a flask. Add approximately 50 ml of water (remember, not tap water) and three drops of methyl red indicator. Fill a 25 ml buret with the 0.1 N sodium hydroxide solution and record the initial volume.

## Why do we use Khp to standardize NaOH?

KHP is slightly acidic, and it is often used as a primary standard for acid-base titrations because it is solid and air-stable, making it easy to weigh accurately. It is not hygroscopic.

## Why do we standardize NaOH with KHP?

Solid NaOH is highly hygroscopic (it absorbs water from the air) and thus it cannot be accurately weighed. A KHP sample of known mass (and, therefore, known moles) can be titrated with the NaOH solution to determine very precisely the concentration of the NaOH. This procedure is called standardizing the NaOH solution.

## How do you standardize NaOH with oxalic acid?

Add about 25 mL of deionized water and 3 drops of phenolphthalein to the oxalic acid. Swirl the mixture to dissolve the oxalic acid. Read the buret to the nearest 0.01 mL, and titrate the oxalic acid with NaOH. The end point has been reached when the pale pink color of the phenolphthalein persists for 30 seconds.

## How do I calculate molar concentration?

Concentration formula: To find the molar concentration of a solution, simply divide the total moles of solute by the total volume of the solution in liters.

## Is Solid NaOH hygroscopic?

Solid sodium hydroxide is hygroscopic, which means that it absorbs moisture from the atmosphere. Once it has a little moisture it also absorbs carbon dioxide which is always present in air.

## How do you find the molarity of NaOH?

First determine the moles of NaOH in the reaction. From the mole ratio, calculate the moles of H2SO4 that reacted. Finally, divide the moles of H2SO4 by its volume to get the molarity.

## How do I calculate the concentration of a solution?

The molarity (M) of a solution is the number of moles of solute dissolved in one liter of solution. To calculate the molarity of a solution, you divide the moles of solute by the volume of the solution expressed in liters. Note that the volume is in liters of solution and not liters of solvent.

## How do you calculate the standardization of HCl?

Pipette 25.00mL of HCl(aq) into a 125mL Ehrlenmeyer flask and add two drops of phenolphthalein indicator. Titrate this solution with NaOH(aq) to the endpoint. Calculate the concentration of the HCl(aq) stock. Repeat this titration until your average result has an error that you consider acceptable.

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