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3 years ago

What is the solubility of a solid in a solvent?

Chemistry

1 answer:

patriot [66]3 years ago

5 0

Answer:

Solubility is a chemical property referring to the ability for a given substance, the solute, to dissolve in a solvent. It is measured in terms of the maximum amount of solute dissolved in a solvent at equilibrium. ... The solvent is often a solid, which can be a pure substance or a mixture.

Explanation:

You might be interested in

What mass of chlorine gas is contained in a 10.0 L tank at 31.0° C and 3.50 atm?

jeyben [28]

You need to use the ideal gas law (PV=nRT) and solve for n. ((3.50atm•10.0L)/(0.0821(L•atm/mol•K)•304K) = n = 1.40 moles. 1 mole of Cl2 = 70.9 gm/mole. The mass would be 99.43 gm

8 0

3 years ago

What stresses will shift the reaction to increase the products

AveGali [126]

Answer:

Change in molarity, temperature, volume/pressure depending on the conditions given

Explanation:

It really depends on the type of a reaction, however, we may apply general trends and see every possibility:

if we increase the concentration of products, then, according to the principle of Le Chatelier, the equilibrium will shift toward the formation of products;
if we have an endothermic reaction, increasing heat will lead a shift to the right and toward formation of products, since heat might be considered a reactant as well;
if we have an exothermic reaction, removing heat/decreasing temperature will lead to an increase in products, as we're removing one of our products, heat, and system will try to rebuild the amount of heat lost forming the other products as a result as well;
if we have gaseous substances in a reaction, an increase in pressure will shift the equilibrium to the right if we have a greater amount in moles of reactant gases compared to products, this is also known as a decrease in volume;
if we have gaseous substances in a reaction, a decrease in pressure will shift the equilibrium to the right if we have a greater amount in moles of product gases compared to reactants, this is also known as an increase in volume.

7 0

2 years ago

What happens to a reducing agent during a redox reaction?

Nuetrik [128]

Reducing agent is an compound/atom, that loses an electron and is oxidized.

0.........+I.............+II............0
Ca + 2HCl ----> CaCl₂ + H₂

Calcium is oxidized --- it's reducing agent (reductant).
Hydrogen is reduced --- HCl is oxidizing agent.

7 0

3 years ago

The pH of 0.10 M solution of an acid is 6. What is the percentage ionization of the acid?

Natasha_Volkova [10]

Hey there!:

HA <=> H⁺ + A⁻

pH = -log[H+] = 6

[ H⁺ ] = 10^-pH

[ H⁺] = 10 ^ -6

[ H⁺ ] = 0.000001 M

Percent dissociation:

[ H⁺ ] / [ HA]o * 100

[ 0.000001 / 0.10 ] * 100

0.00001 * 100 => 0.0010%

Answer D

Hope that helps!

6 0

2 years ago

In the laboratory you dissolve 22.0 g of nickel(II) nitrate in a volumetric flask and add water to a total volume of 125

Ahat [919]

Answer:

<u>1.364 M</u>.

Explanation:

Molarity formula: M= n/v, where n is moles of solute, and v is liters of solution.

Now, we need to convert the grams of nickel to moles and the volume of water to liters.

125mL/1000= 0.125 L.

To convert nickel grams to moles, we need to take a look at it's chemical formula, which is:

$Ni(NO_{3} )_{2}$

Now we count how many molecules of each element we have:

Ni= 1

N= 2

O= 6

Calculate the weight (g) of each element (the values of g/mol can be found on the periodic table and they may vary slightly between one table and the other):

Ni: (1) (58.6934)= 58.6934

N= (2) (14.007)= 28.014

O= (6) (15.999)= 95.994

Sum all the values to obtain the total weight of 1 mole of this compound:

58.6934+28.014+95.994= 129(g/mole)

Now that we know the that 129 grams equal 1 mole of nickel(II) nitrate, we can convert the 22.0 g to moles:

129g ------- 1 mole

22.0g ----- x

x= (22*1)/129= 0.1705 moles.

Now, we have all the values needed to calculate the molarity of this solution. All we have to do is substitute the values in the formula:

M= (0.1705 moles) / (0.125 L)= <u>1.364 M</u>.

3 0

1 year ago