Chemistry High School

How is bleaching powder prepared???

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Answers

Answer 1

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How is bleaching powder prepared?

It is prepared by the action of chlorine gas on dry slaked lime Ca(OH)²

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[tex] \dag \boxed{\red{\sf{Ca(OH) {}^{2} +cl {}^{2} →CaOCl {}^{2} +H {}^{2} O}}}[/tex]

Related Questions

The liquid dispensed from a burette is called ___________.

i. solute

ii. water

iii. titrant

iv. analyte

Answers

The liquid dispensed from a burette is called the titrant. A titrant is a solution with a known concentration that is added in a controlled manner to react with the analyte in a chemical analysis. The option C is correct.

The burette is a precise measuring instrument used in titrations to deliver the titrant.In a titration, the analyte is the substance being analyzed or tested. It reacts with the titrant to form a product, and the reaction is monitored to determine the concentration or amount of the analyte.

For example, in an acid-base titration, a solution of known concentration called the titrant is slowly added to the analyte solution until the reaction between the acid and base is complete. The burette allows for precise measurement of the volume of titrant added.The other options given are not accurate in this context. Solute refers to the substance being dissolved in a solvent, while water is a common solvent. Analyte, as mentioned earlier, is the substance being analyzed. The correct term for the liquid dispensed from a burette in a titration is the titrant.

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at constant temperature, a 144.0 ml sample of gas in a piston chamber has a pressure of 2.25 atm. calculate the pressure of the gas if this piston is pushed down hard so that the gas now has a volume of 36.0 ml.

Answers

The pressure of the gas would be 9.0 atm if the piston is pushed down hard to a volume of 36.0 ml.

To solve this problem, we can use Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume at constant temperature.

First, we need to set up the equation: P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.

Given that the initial volume (V1) is 144.0 ml and the initial pressure (P1) is 2.25 atm, and the final volume (V2) is 36.0 ml, we can plug in the values into the equation:

2.25 atm * 144.0 ml = P2 * 36.0 ml

Next, we can solve for P2 by dividing both sides of the equation by 36.0 ml:

2.25 atm * 144.0 ml / 36.0 ml = P2

P2 = 9.0 atm

Therefore, the pressure of the gas would be 9.0 atm if the piston is pushed down hard to a volume of 36.0 ml.

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