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EleoNora [17]
2 years ago
10

At what temperature would a 1.50 m nacl solution freeze, given that the van't hoff factor for nacl is 1.9? kf for water is 1.86

∘c/m .
Chemistry
1 answer:
IRINA_888 [86]2 years ago
5 0
Win to ki ne lei ma ki mna mata ki ss kk
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Likurg_2 [28]

Answer:

skeletal, smooth, and cardiac muscles

Explanation:

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3 years ago
One mole of a metallic oxide reacts with one mole of hydrogen to produce two moles of the pure metal
MAXImum [283]

Answer:

The metallic oxide is Li₂O

Explanation:

Let the metallic oxide be M₂O

Thus;

M₂O + H₂ = 2M + H₂O

Molar mass of M₂O = (2x + 16)

We assume Molar mass of M to be x.

We are told that 5.00 g of the metallic oxide produces 2.32 g of the metal.

By proportion, we can write the following;

5g of M₂O × (1 mole of M₂O/(2x + 16)) × (2 moles of M/1 mole of M₂O) = 2.32 g of M × 1 mole of M/x g of M

This cancels out to give us;

10/(2x + 16) = 2.32/x

Cross multiply to get;

10x = 2.32(2x + 16)

10x = 4.64x + 37.12

10x - 4.64x = 37.12

5.36x = 37.12

x = 37.12/5.36

x = 6.925 g/mol

The metal with a molar mass closest to this value of x is Lithium which has a molar mass of 6.94 g/mol

Thus the metal is Lithium and as such the metallic oxide is Li₂O

6 0
2 years ago
Calculate the change in ph when 3.00 ml of 0.100 m hcl(aq) is added to 100.0 ml of a buffer solution that is 0.100 m in nh3(aq)
nikklg [1K]

The change in pH is calculated by:

pOH = Protein kinase B + log [NH4+]/ [NH3] 

Protein kinase B of ammonia = 4.74 

initial potential of oxygen hydroxide= 4.74 + log 0.100/0.100 = 4.74 
pH = 14 - 4.74=9.26 

moles NH4+ = moles NH3 = 0.100 L x 0.100 M = 0.0100 
moles H+ added = 3.00 x 10^-3 L x 0.100 M=0.000300 

NH3 + H+ = NH4+ 
moles NH3 = 0.0100 - 0.000300=0.00970 
moles NH4+ = 0.0100 + 0.000300=0.0103 

pOH = 4.74 + log 0.0103/ 0.00970= 4.77 
oH = 14 - 4.77 = 9.23 

the change is  = 9.26 - 9.23 =0.03 

7 0
3 years ago
What is the process of using one or more of your five senses to measure or collect data?
sveta [45]

Answer:

B no observation pls mark me branilest

7 0
2 years ago
Read 2 more answers
How many grams of sulfur must be burned to give 100.0 g of So2
andriy [413]

Answer:

50 g of S are needed

Explanation:

To star this, we begin from the reaction:

S(s) + O₂ (g) →  SO₂ (g)

If we burn 1 mol of sulfur with 1 mol of oxygen, we can produce 1 mol of sulfur dioxide. In conclussion, ratio is 1:1.

According to stoichiometry, we can determine the moles of sulfur dioxide produced.

100 g. 1mol / 64.06g = 1.56 moles

This 1.56 moles were orginated by the same amount of S, according to stoichiometry.

Let's convert the moles to mass

1.56 mol . 32.06g / mol = 50 g

4 0
2 years ago
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