0.28 g of CaCO3 was dissolved in HCl and the solution made upto 1litre of water. 100 ml of the above solution required 28 ml of EDTA solution on titration. 100 ml of hard water sample required 33ml of same required solution on titration. After 100ml of this water, cooling and filtering and then titrated 10ml of EDTA solution. Calculate the temporary and permanent hardnes.

The problem is about calculating the temporary and permanent hardness of water using titration data. Here are the steps to solve it:

1. First, calculate the amount of CaCO3 that reacts with 1 ml of EDTA. Since 0.28 g of CaCO3 reacts with 28 ml of EDTA, 1 ml of EDTA will react with 0.28/28 = 0.01 g of CaCO3.

2. Next, calculate the amount of CaCO3 in the 100 ml hard water sample. Since 33 ml of EDTA is required to titrate the 100 ml hard water sample, the amount of CaCO3 in the 100 ml hard water sample is 33 * 0.01 = 0.33 g.

3. The total hardness of the water is given by the amount of CaCO3 in the 100 ml sample, which is 0.33 g. To convert this to mg/l (ppm), multiply by 10 (since 100 ml is 1/10 of a litre), giving a total hardness of 0.33 * 10 = 3.3 mg/l.

4. After boiling, cooling and filtering the water, 10 ml of EDTA is required to titrate the water. This means that the amount of CaCO3 in the water after boiling is 10 * 0.01 = 0.1 g. To convert this to mg/l, multiply by 10, giving a hardness after boiling of 0.1 * 10 = 1 mg/l.

5. The temporary hardness is the difference between the total hardness and the hardness after boiling, which is 3.3 - 1 = 2.3 mg/l.

6. The permanent hardness is the hardness after boiling, which is 1 mg/l.