Home
Class 11
CHEMISTRY
A hard water sample has 131 ppm CaSO(4)....

A hard water sample has `131` ppm `CaSO_(4)`. What fraction of the water must be evaporated in a container before solid `CaSO_(4)` begins to deposit. `K_(sp) of CaSO_(4) = 9.0 xx 10^(-6)`.

Text Solution

AI Generated Solution

To solve the problem of determining the fraction of water that must be evaporated from a hard water sample containing 131 ppm of CaSO₄ before solid CaSO₄ begins to deposit, we will follow these steps: ### Step 1: Calculate the solubility of CaSO₄ using Ksp The solubility product constant (Ksp) for CaSO₄ is given as \(9.0 \times 10^{-6}\). The dissociation of CaSO₄ in water can be represented as: \[ \text{CaSO}_4 (s) \rightleftharpoons \text{Ca}^{2+} (aq) + \text{SO}_4^{2-} (aq) \] ...
Promotional Banner

Similar Questions

Explore conceptually related problems

100 ml sample is removed from a water solution with CaSO_(4) at 25^(@)C . The water is completely evaorated from the sample and deposit of 0.24 gm CaSO_(4) is obtained . What is K_(sp) for CaSO_(4) at 25^(@)C

What is the solubility of PbSO_(4) in 0.01M Na_(2)SO_(4) solution if K_(sp) for PbSO_(4) = 1.25 xx 10^(-9) ?

A sample of hard water contains 0.05mol of CaC1_(2) , per litre, What is the minimum concentration of Na_(2)SO_(4) , which must be added for removing Ca^(2+) ions from this water sample? K_(sp) for CaSO_(4) is 2.4 xx 10^(-5) at 25^(@)C .

What happens when hard water containing CaSO_(4) is treated with calgon.

One litre sample of hard water contains 0.006 mole CaCl_2 . The minimum concentration of Na_2SO_4 needed for the precipitation of CaSO_4 is ( K_(sp) for CaSO_4 is 3.0xx10^-6 at 25^oC )

You are provided with 500mL of hard water, containing 0.005 mol of CaC1_(2) and two H_(2)SO_(4) samples of 0.001M and 0.02M concentration. Which one or both or none can be used for precipitating Ca^(2+) ions. K_(sp) of CaSO_(4) = 2.4 xx 10^(-4) .

A solution contains 0.1M each of CaCI_(2) and SrCI_(2). A 0.005M solution of SO_(4)^(2-) is slowly added to the given solution. a. Which substance beings to precipiate first? b. If H_(2)SO_(4) is continuosult added, determine when will other salt be precipitated? c. When second salt starts to precipitate, find the concentration of cation of first salt. Assume that CaCI_(2) and SrCI_(2) are 100% ionised and volume of the solution remains constant. K_(sp) of SrSO_(4) = 3.2 xx 10^(-7) and K_(sp)of CaSO_(4) = 1.3 xx 10^(-4)

the hardness of a water sample (in terms of Equivalents of CaCO_(3) ) containing 10^(-3)MCaSO_(4) Is : (Molar mass of CaSO_(4)=136 gmol^(-1) )

Hydrated calcium sulphate has the formula of CaSO_4 . 2H_2O . What is the name given to the water molecules present in the salt ?

What is minimum concentration of SO_(4)^(2-) required to precipitate BaSO_(4) in solution containing 1 xx 10^(-4) mole of Ba^(2+) ? ( K_(sp) of BaSO_(4) = 4 xx 10^(-10) )