1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
IrinaVladis [17]
3 years ago
10

HELP PLEASE. 20 POINTS AND BRAINLIEST!!!! Solubility of salts in water is temperature dependent. Consider the solubility curve o

f the salts seen here. Which salt's solubility changed the least from 0 - 100oC; which salt's solubility changed the greatest amount from 0 - 100oC?

Chemistry
2 answers:
Zina [86]3 years ago
6 0

Answer: Sodium chloride's solubility has changed the least from  0^0C-100^0C and potassium nitrate's solubility has changed the most from 0^0C-100^0C.

Explanation:

Solubility in a particular liquid is the amount of solute that can dissolve in unit volume of the liquid to form the saturated solution at the given temperature and under a pressure of 1 atmosphere.

a) Solubility of Potassium iodide at 0^0C: 129g/100 ml

Solubility of Potassium iodide at 100^0C: 250g/10ml

Change in solubility of Potassium iodide = (250-129)^0C=121^0C

b) Solubility of sodium nitrate at 0^0C: 70g/100 ml

Solubility of sodium nitrate at 100^0C: 180 g/100 ml

Change in solubility of sodium nitrate  = (180-70)^0C=110^0C

c) Solubility of Potassium nitrate at 0^0C: 12g/100 ml

Solubility of Potassium nitrate at 100^0C: 235g/100 ml

Change in solubility of Potassium nitrate = (235-12)^0C=223^0C

d) Solubility of sodium chloride at 0^0C: 36g/100 ml

Solubility of sodium chloride at 100^0C: 40 g/100 ml

Change in solubility of sodium chloride= (40-36)^0C=4^0C

e) Solubility of Potassium chlorate at 0^0C: 5g/100 ml

Solubility of Potassium chlorate at 100^0C: 60 g/100 ml

Change in solubility of Potassium chlorate = (60-5)^0C=55^0C

Thus we can see that sodium chloride's solubility has changed the least from  0^0C-100^0C and potassium nitrate's solubility has changed the most from 0^0C-100^0C.

Dennis_Churaev [7]3 years ago
4 0
Sodium chloride's solubility only changed about 5 g/100 mL water, whereas potassium nitrate's solubility changed about 230 g/100 mL water
You might be interested in
Find the enthalpy of neutralization of HCl and NaOH. 137 cm3 of 2.6 mol dm-3 hydrochloric acid was neutralized by 137 cm3 of 2.6
liraira [26]

Answer : The correct option is, (D) 89.39 KJ/mole

Explanation :

First we have to calculate the moles of HCl and NaOH.

\text{Moles of HCl}=\text{Concentration of HCl}\times \text{Volume of solution}=2.6mole/L\times 0.137L=0.3562mole

\text{Moles of NaOH}=\text{Concentration of NaOH}\times \text{Volume of solution}=2.6mole/L\times 0.137L=0.3562mole

The balanced chemical reaction will be,

HCl+NaOH\rightarrow NaCl+H_2O

From the balanced reaction we conclude that,

As, 1 mole of HCl neutralizes by 1 mole of NaOH

So, 0.3562 mole of HCl neutralizes by 0.3562 mole of NaOH

Thus, the number of neutralized moles = 0.3562 mole

Now we have to calculate the mass of water.

As we know that the density of water is 1 g/ml. So, the mass of water will be:

The volume of water = 137ml+137ml=274ml

\text{Mass of water}=\text{Density of water}\times \text{Volume of water}=1g/ml\times 274ml=274g

Now we have to calculate the heat absorbed during the reaction.

q=m\times c\times (T_{final}-T_{initial})

where,

q = heat absorbed = ?

c = specific heat of water = 4.18J/g^oC

m = mass of water = 274 g

T_{final} = final temperature of water = 325.8 K

T_{initial} = initial temperature of metal = 298 K

Now put all the given values in the above formula, we get:

q=274g\times 4.18J/g^oC\times (325.8-298)K

q=31839.896J=31.84KJ

Thus, the heat released during the neutralization = -31.84 KJ

Now we have to calculate the enthalpy of neutralization.

\Delta H=\frac{q}{n}

where,

\Delta H = enthalpy of neutralization = ?

q = heat released = -31.84 KJ

n = number of moles used in neutralization = 0.3562 mole

\Delta H=\frac{-31.84KJ}{0.3562mole}=-89.39KJ/mole

The negative sign indicate the heat released during the reaction.

Therefore, the enthalpy of neutralization is, 89.39 KJ/mole

3 0
3 years ago
Please answer for brainliest and if your answer is correct I'll give extra points. screenshot of the question is below.
ozzi

Concentration - 3

Phase - 1

Catalyst - 4

Surface area - 2

8 0
2 years ago
Read 2 more answers
A student placed a crystal of a blue dye at the bottom of a beaker of water. After 5 minutes, the crystal sa
ludmilkaskok [199]

Explanation:

It is because it is having color in it  and the water is colorless

7 0
2 years ago
Rainwater can have a ph as low as 3,meaning that it is very
GREYUIT [131]

Rainwater can have a ph as low as 3, meaning that it is very C. Acidic

3 0
3 years ago
Sugar dissolves when stirred into coffee. The coffee is the ________, the sugar is the ________, and the sweetened coffee is the
Finger [1]

Answer:

The coffee is the solvent. The sugar is the solute. The sweetened coffee is the solution.

Explanation:

8 0
2 years ago
Other questions:
  • Which type of chemical model shows the bond angle and bond length between atoms and compounds?
    6·1 answer
  • How can you increase the amount of work done when you lift a book explain
    15·1 answer
  • What kind of bond holds together atoms within a molecule?
    7·2 answers
  • How many carbons are in a molecule of hexane?<br> a. 2<br> b. 4<br> c. 6<br> d. 8
    14·1 answer
  • Please everyone do this and send me​
    12·1 answer
  • How many atoms in Alka-Seltzer
    8·2 answers
  • A carpenter uses a saw to cut a wooden board into two different sized pieces. Which of the following physical properties is most
    10·2 answers
  • When light waves pass through solids, the speed of the wave ___________.
    11·1 answer
  • What are the most of the elements in the periodic table
    5·2 answers
  • Calculate the root mean square velocity, in m/s, of carbon dioxide molecules at 100.0
    14·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!