Home
Class 11
CHEMISTRY
A 100 mL of tap water was titrated with ...

A `100 mL` of tap water was titrated with `M//50 HCl` with methyle orange as indicator. If `30 mL of HCl` were required. Calculate the hardness of `CaCO_(3)` per `10^(3)` parts of water. The hardness is temporary.

A

`150 "ppm"`

B

`600 "ppm"`

C

`275 "ppm"`

D

`300 "ppm"`

Text Solution

Verified by Experts

The correct Answer is:
D
Meq. of `CaCO_(3)`= Meq. of `Ca(HCO_(3))_(2)` = Meq. of HCl
`(W)/(100//2)xx 1000= (1)/(50) xx 30`
`W_(CaCO_(3))= (3 xx 100 )/(5 xx 2000) = 0.03 g`
`therefore 100 mL " of "H_(2)O " contins " Ca^(2+)= (0.03 xx 10^(6))/(100)= 300 "ppm"`
Promotional Banner

Topper's Solved these Questions

  • HYDROGEN

    BITSAT GUIDE|Exercise BITSAT Archives|5 Videos

  • CHEMICAL BONDING

    BITSAT GUIDE|Exercise BITSAT Archives|14 Videos

  • NUCLEAR CHEMISTRY

    BITSAT GUIDE|Exercise BITSAT Archives|4 Videos

Similar Questions

Explore conceptually related problems

100 mL of tap water containing Ca(HCO_3)_2 was titrated with N/50 HCl with methyl orange as indicator. If 30 mL of HCl were required, calculate the temporary hardness as parts of CaCO_3 per 10^6 parts of water.

50 ml of water sample requires 10 ml of (M)/(50)HCl for complete neutralization. Calculate hardness of H_(2)O (temporary) in ppm.

10 L of hard water requires 0.28 g of line (CaO) for removing hardness. Calculate the temporary hardness in ppm of CaCO_(3) .