Home
Class 12
CHEMISTRY
The use of common salts, e.g., NaCl or C...

The use of common salts, e.g., `NaCl` or `CaCl_(2)` anhydrous, is made to clear snow on the roads. This causes:

A

A lowering in the freezing point of water.

B

A lowering in the melting point of ice.

C

Ice melts at the temperature of atmosphere present at that time.

D

All of these

Text Solution

Verified by Experts

The correct Answer is:
D
Addition of salt lowers the freezing point of water and thus snow melts.
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • SOLUTIONS

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercise (Assertion-Reasoning)|18 Videos

  • SOLUTIONS

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercise (Interger)|8 Videos

  • SOLUTIONS

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercises (Multiple Correct)|25 Videos

  • SOLID STATE

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 1.2 (Objective)|9 Videos

  • SURFACE CHEMISTRY

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|2 Videos

Similar Questions

Explore conceptually related problems

Sodium choride or calcium chloride is used to clear snow from the roads. Why?

Read following statement(s) carefully and select the right option : (I) The enthalpy of solution of CaCl_(2). 6H_(2)O in a large volume of water is endothermic to the extent of 3.5 kcal/mol. If DeltaH=-23.2 " kcal" for the reaction, CaCl_(2)(s)+6H_(2)O(l)rarrCaCl_(2).6H_(2)O(s) then heat of solution of CaCl_(2) (anhydrous) in a large volume of water is - 19.7 kcal/mol (II) For the reaction 2Cl(g)rarrCl_(2)(g) , the sign of DeltaH and DeltaS are negative.

10 g of a sample of a mixture of CaCl_(2) and NaCl is treated to precipitate all the calcium as CaCO_(3) . This CaCO_(3) is heated to convert all the Ca to CaO and the final mass of CaO is 1.62 g.The percent by mass of CaCl_(2) in the origial mixture is

0.378 g of an organic compound containing carbon and hydrogen was subjected to combustion by Liebig's method , the CO_(2) and H_(2)O formed were passed through potash bulbs and CaCl_(2) (anhydrous) tube. At end of the experiment, the increase in the respective weights were 0.264 g and 0.162 g. Calculate the percentage of carbon and hydrogen.

Sodium metal can be extracted by either Castner's Process or Down's process Castner's process. Electrolyte to fused NaOH Cathode and anode are made up of a steel rod and Ni cylinder respectively the reaction takes place as follows : At cathode Na^(+)+e^(-)toNa At anode OH^(-)to(1)/(2)H_(2)O+(1)/(4)O_(2)uarr+e^(-) Down's process : Electrolyte to fused NaCl and CaCl_(2) Cathode and anode are ring shaped iron metal and graphite respectively. The reaction takes place as follows : Na^(+)+e^(-)toNa Cl^(-)to(1)/(2)Cl_(2)uarr+e^(-) CaCl_(2) is used along with NaCl due to

Dow's process of extraction of Mg involves extraction of Mg from sea water. Sea water is concentrated in sun-light and is then treated with slaked lime. Magnesium hydroxide is heated in a stream of HCl to give MgCl_(2) which is electrolysed to discharge Mg. The mixture is in the ratio 35% MgCl_(2)+50% NaCl+15% CaCl_(2) . NaCl and CaCl_(2) are added to lower the fusion temperature and to increases the conductance. Mg^(2+) +Ca(OH)_(2) to Mg(OH)_(2)+Ca^(2+) Mg(OH)_(2)+2HCl to MgCl_(2)+2H_(2)O(l) Electrolysis of fused MgCl_(2) hArr Mg^(2+)+2Cl Mg^(2+)+2e^(-) to Mg ( At Cathode) 2Cl^(-) to Cl_(2)+2e^(-) (At Anode) Mg electrolysed is protected from atmospheric oxidation by a blanket of inert gases. Molten mixutre of NaCl and CaCl_(2) is added to the heated MgCl_(2) because :

CaCl_(2) is preferred over NaCl for clearing ice on roads particularly in very cold countries. This is because:

CaCl_(2) is preferred over NaCl for clearing ice on roads particularly in very cold countries. This is because:

Dow's process of extraction of Mg involves extraction of Mg from sea water. Sea water is concentrated in sun-light and is then treated with slaked lime. Magnesium hydroxide is heated in a stream of HCl to give MgCl_(2) which is electrolysed to discharge Mg. The mixture is in the ratio 35% MgCl_(2)+50% NaCl+15% CaCl_(2) . NaCl and CaCl_(2) are added to lower the fusion temperature and to increases the conductance. Mg^(2+) +Ca(OH)_(2) to Mg(OH)_(2)+Ca^(2+) Mg(OH)_(2)+2HCl to MgCl_(2)+2H_(2)O(l) Electrolysis of fused MgCl_(2) hArr Mg^(2+)+2Cl Mg^(2+)+2e^(-) to Mg ( At Cathode) 2Cl^(-) to Cl_(2)+2e^(-) (At Anode) Mg electrolysed is protected from atmospheric oxidation by a blanket of inert gases. In the hydrated chloride of Mg the value of x is :

Dow's process of extraction of Mg involves extraction of Mg from sea water. Sea water is concentrated in sun-light and is then treated with slaked lime. Magnesium hydroxide is heated in a stream of HCl to give MgCl_(2) which is electrolysed to discharge Mg. The mixture is in the ratio 35% MgCl_(2)+50% NaCl+15% CaCl_(2) . NaCl and CaCl_(2) are added to lower the fusion temperature and to increases the conductance. Mg^(2+) +Ca(OH)_(2) to Mg(OH)_(2)+Ca^(2+) Mg(OH)_(2)+2HCl to MgCl_(2)+2H_(2)O(l) Electrolysis of fused MgCl_(2) hArr Mg^(2+)+2Cl Mg^(2+)+2e^(-) to Mg ( At Cathode) 2Cl^(-) to Cl_(2)+2e^(-) (At Anode) Mg electrolysed is protected from atmospheric oxidation by a blanket of inert gases. Molten mixture contains Mg^(2+), Na^(+) and Ca^(2+) but at cathode only Mg^(2+) is discharged because :

Home
Profile