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Multiple choice evs experiments with water water and its types hard and soft water what floats - what sinks

Which one of the following process will produce hard water?

  1. Saturation of water with $MgCO _{3}$
  2. Saturation of water with $CaSO _{4}$
  3. Addition of $Na _{2}SO _{4}$ to water
  4. Saturation of water with $CaCO _{3}$
Reveal answer Fill a bubble to check yourself
B Correct answer
Explanation

Calcium sulfate $\left( CaS{ O } _{ 4 } \right) $ being less soluble in water causes permanent hardness in water.

Multiple choice evs experiments with water water and its types hard and soft water what floats - what sinks

Unstable hardness of water is due to the presence of:

  1. $CaCl _{2},\:MgSO _{4}$
  2. $Ca^{+2},\:Mg^{+2}$
  3. $K^{+},\:CaCO _{3}$
  4. $Ca(HCO _{3}) _{2},\:Mg(HCO _{3}) _{2}$
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Hard water, water that contains salts of calcium and magnesium principally as bicarbonates, chlorides, and sulfates. Water hardness that is caused by calcium bicarbonate is known as temporary, because boiling converts the bicarbonate to the insoluble carbonate; hardness from the other salts is called permanent.

Multiple choice evs experiments with water water and its types hard and soft water what floats - what sinks

In a sample of temporary hard water which of the following water softening process does NOT produced any precipitate of cation responsible for hardness ? 

  1. Boiling water

  2. Addition of lime water

  3. Addition of sodium hexameta phosphate

  4. Addition of sodium carbonate
Reveal answer Fill a bubble to check yourself
C Correct answer
Explanation

Temporary hardness is caused by bicarbonates of calcium and magnesium. Boiling water precipitates insoluble carbonates. Adding lime water precipitates calcium carbonate or magnesium hydroxide. Adding sodium carbonate precipitates calcium carbonate. However, adding sodium hexametaphosphate (Calgon's method) sequesters the calcium and magnesium ions into soluble complex anions without forming any precipitate of the hardness-causing cations.

Multiple choice evs experiments with water water and its types hard and soft water what floats - what sinks

One litre hard water contains $12 mg\, Mg^{2+}$ milli-equivalent of washing soda required to remove its hardness is: 

  1. $1$
  2. $12.16$
  3. $1\times 10^{-3}$
  4. $12.16\times 10^{-3}$
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation

The molar mass of Mg2+ is 24 g/mol. 12 mg is 0.5 millimoles. Since Mg2+ has a valency of 2, this corresponds to 1 milliequivalent. Washing soda (Na2CO3) reacts in a 1:1 equivalent ratio to remove the hardness.

Multiple choice evs experiments with water water and its types hard and soft water what floats - what sinks

Which of the following pair of ions makes the water hard?

  1. $Na^+,SO _4^{+2}$
  2. $Ca^{2+},HCO _3^-$
  3. $Ca^{2+},NO _3$
  4. $NH _4^-,Cr$
Reveal answer Fill a bubble to check yourself
B Correct answer
Explanation

Causes

1) High mineral (calcium and magnesium) content.
2) It can be found in groundwater as it passes through lime.
Types 
1) Permanent: It is caused due to the presence of sulphate and chloride salts.  Heating does not remove the permanent hardness of water so it is treated with chemicals.  Resins or water softeners are used to remove the permanent hardness.
2) Temporary: It is caused due to the presence of bicarbonate salts.  It can easily be removed by boiling.  Boiling decomposes the salts into insoluble carbonates.  Water can also be treated with calcium hydroxide to remove the hardness.Water Hardeners are Ca2+ and HCO3.   Nitrates and sulfates are used as water softener.  

Multiple choice evs experiments with water water and its types hard and soft water what floats - what sinks

In water:

  1. temporary hardness is due to the bicarbonates of $Ca^{2+}$ and $Mg^{2+}$.
  2. permanent hardness is due to chlorides and sulphates of $Ca^{2+}$ and $Mg^{2+}$.

  3. hardness can be removed by adding phosphates.

  4. all of the above.
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Temporary hardness is indeed due to bicarbonates, permanent hardness is due to chlorides/sulfates, and phosphates are used in water softening processes (like Calgon).

Multiple choice evs experiments with water water and its types hard and soft water what floats - what sinks

$Na _2CO _3$ is widely used in softening of hard water. If 1 L of hard water required $0.0106 g$ of $Na _2CO _3$, The hardness in ppm (parts per million i.e., $10^{6}$ ml) of $CaCO _3$ is:

  1. $0.01\,$ ppm $CaCO _3$
  2. $0.10\,$ ppm $CaCO _3$
  3. $1.00\,$ ppm $CaCO _3$
  4. $10.00\,$ ppm $CaCO _3$
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Hardness (in ppm)=$\cfrac {Weight\quad of\quad Na _2CO _3\quad required\quad (in\quad mg)}{Volume\quad of\quad Hard\quad water\quad (in\quad L)}$

=$\cfrac {0.0106\times 10^{3}}{1}$
=$10.6$
$\approx 10 ppm$
$\therefore$ Hardness (in ppm)= $10$ ppm $CaCO _3$

Multiple choice evs experiments with water water and its types hard and soft water what floats - what sinks

A volume of 100 L of hard water requires 5.6 g of lime for removing temporary hardness. The temporary hardness in ppm of CaCO3CaCO3 is:

  1. 56

  2. 100

  3. 200

  4. 112
Reveal answer Fill a bubble to check yourself
C Correct answer
Explanation

Temporary hardness is amount of $ CaCO _{3} $ in grams present in $ 10^{6}\,ml/grams $ of water


$ Ca(HCO _{3}) _{2}+CaO\rightarrow 2CaCO _{3}+H _{2}O $

$ 56\,g  $                      $ 2\times 100 = 200\,g $

$ 5.6\,g $                      $ 20\,g $ 

20 g $ CACO _{3} $ present in 100 L $ H _{2}O $

$ = 100\times 10^{3} = 10^{5}\,ml $

Then $ 10^{6} $ ml water contains 200g $ CaCO _{3} $

$ \therefore $ 200 ppm is temporary hardness 

Hence, the correct option is $\text{C}$.