You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Avogadro's Law & Gay Lussac's Law

The freezing ...

Question

The freezing point depression constant for water is $- 1.86 ° C m^{- 1}$ . If 5.00 g $N a_{2} S O_{4}$ is dissolved in $45.0 g$ $H_{2} O$ , the freezing point is changed by $- 3.82 ° C$ . Calculate the van’t Hoff factor for $N a_{2} S O_{4}$ .

2.05

No worries! We‘ve got your back. Try BYJU‘S free classes today!

0.381

No worries! We‘ve got your back. Try BYJU‘S free classes today!

2.63

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

3.11

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is C 2.63
We know that,
$Δ T_{f} = i \times K_{f} \times \frac{w_{B} \times 1000}{M_{B} \times W_{A}}$
Given : $Δ T_{f} = 3.82 ° C, K_{f} = 1.86 ° C m^{- 1}, w_{B} = 5 g, M_{B} = 142 g, W_{A} = 45 g$
$i = \frac{Δ T_{f} \times M_{B} \times W_{A}}{K_{f} \times w_{A} \times 1000} = \frac{3. 82 \times 142 \times 45}{186 \times 5 \times 1000} = 2.63$

Suggest Corrections

Similar questions

Q. The freezing point depression constant for water is

- {1.86}^{0} C m^{- 1} .

If 5.00 g

N a_{2} S O_{4}

is dissolved in 45.0 g

H_{2} O,

the freezing point is changed by

{3.82}^{0} C .

Calculate the vant Hoff factor for

N a_{2} S O_{4} .

Q. The freezing point depression constant for water ids

{1.86}^{o} c m^{- 1}

. If

5.0

g of

N a_{2} S O_{4}

is dissolved in

45.0

H_{2} O

, the freezing point is change by

- {3.82}^{o} C

. Calculate the van't Hoff factor for

N a_{2} S O_{4}

Q. The freezing point depression constant for water is

{1.86}^{o} C

m^{- 1}

. If

5

N a_{2} S O_{4}

is dissolved in 45 g

H_{2} O

, the freezing point is changed by

- {3.82}^{o} C

Calculate the van't Hoff factor for

N a_{2} S O_{4}

Q. If

5 g

N a_{2} S O_{4}

is dissolved in

45 g

H_{2} O

, the freezing point is changed by

{3.72}^{\circ} C

. Calculate the van't Hoff factor for

N a_{2} S O_{4}

.
Given: Freezing point depression constant for water is

{1.86}^{\circ} C k g m o l^{- 1}

Q. Calculate the freezing point depression expected for

0.0711

m aqueous solution of

N a_{2} S O_{4}

. If this solution actually freezes at

- {0.320}^{o}

C, what would be the value of van't Hoff factor? (

K_{f}

for water is

1.86

K kg

m o l^{- 1}

Join BYJU'S Learning Program

The freezing point depression constant for water is –1.86°Cm–1. If 5.00 g Na2SO4 is dissolved in 45.0 g H2O, the freezing point is changed by –3.82°C. Calculate the van’t Hoff factor for Na2SO4.

The correct option is C 2.63We know that, ΔTf=i×Kf×wB×1000MB×WA Given : ΔTf=3.82 °C, Kf=1.86 °Cm–1, wB=5 g, MB=142 g, WA=45 g i=ΔTf×MB×WAKf×wA×1000=3.82×142×45186×5×1000=2.63

The freezing point depression constant for water is $- 1.86 ° C m^{- 1}$ . If 5.00 g $N a_{2} S O_{4}$ is dissolved in $45.0 g$ $H_{2} O$ , the freezing point is changed by $- 3.82 ° C$ . Calculate the van’t Hoff factor for $N a_{2} S O_{4}$ .