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What is the KSP of agcro4?

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What is the KSP of agcro4?

1.2 x 10-12
But first: A 10-minute bonus quiz! Silver chromate, Ag2CrO4 , a sparingly soluble compound, has a solubility product, Ksp , of 1.2 x 10-12 .

How do you calculate solubility?

Solubility indicates the maximum amount of a substance that can be dissolved in a solvent at a given temperature. Such a solution is called saturated. Divide the mass of the compound by the mass of the solvent and then multiply by 100 g to calculate the solubility in g/100g .

What is the KSP formula?

Next we write out the expression for Ksp , then “plug in” the concentrations to obtain the value for Ksp. Let’s do an example: The solubility of Ag2CrO4 in water is 1.31 x 10-4 moles/L. Calculate the value of Ksp . Using mole ratios, the [Ag+] will go up by (2 x 1.31 x 10-4 moles/L) = 2.62 x 10-4 moles/L.

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Is agcro4 soluble?

Although Ag2CrO4 is insoluble in water, it is soluble in dilute HNO3.

What is the solubility class 9?

Amount of a substance (called the solute) that dissolves in a unit volume of a liquid substance (called the solvent) to form a saturated solution under specified conditions of temperature and pressure. Solubility is expressed usually as moles of solute per 100 grams of solvent.

What is solubility in chemistry class 9?

What is Solubility? The maximum amount of solute that can dissolve in a known quantity of solvent at a certain temperature is its solubility. A solution is a homogeneous mixture of one or more solutes in a solvent.

What is the Ksp for a sparingly soluble Ag2CrO4?

The Ksp for a sparingly soluble Ag2CrO4 is 4 × 10^-12 . The molar solubility of the salt is: > The Ksp for a sparingly sol…

How do you calculate the solubility of Ag2CrO4?

Calculate the solubility of Ag2CrO4 A g 2 C r O 4 ( Ksp K s p = 9.0 x 10−12 10 − 12 ) in a 0.069 M AgN O3 A g N O 3 solution.

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What is the K sp of AgCl in AgBr?

The K sp for AgCl is 1.8 x 10 -10. If Ag + and Cl – were both present at 0.0001 M, would a precipitate occur? Iron (III) nitrate has a solubility of 0.15 M. Find concentration of the ions in solution. Calculate [Ag + ], when 0.03 mole of KBr is added to one liter saturated solution of AgBr.

What is the molar solubility of AgCl and Ag(NH3)?

The Ksp for AgCl is 1.6 x 10^-10 and the Kf for Ag (NH3) 2+= 1,5*10^7. Let the molar solubility be C.