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olganol [36]
2 years ago
14

Is salt and water suspension​

Chemistry
2 answers:
mars1129 [50]2 years ago
6 0

Answer:

nah

Explanation:

l though Most Salt are soluble in water (Properties of Ionic Compound) , Not all are soluble ,which means mixing a salt and water can produce either a Solution (homogeneous mixture) or a Suspension (heterogeneous mixture).

swat322 years ago
3 0

Answer:

Solution

Explanation:

The solved dissolves on the solute, creating a homogeneous substance

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438,12 cubic centimeters
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2. An element is all the way through,​
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Submit What is the solubility of Cd3(POA) 2 in water? (Ksp of Cd3(PO4)2 is 2.5 x 10-33) | 1 2 3 +/- . 0 x100
vesna_86 [32]

<u>Answer:</u> The solubility of Cd_3(PO_4)_2 in water is 1.18\times 10^{-7}mol/L

<u>Explanation:</u>

The balanced equilibrium reaction for the ionization of cadmium phosphate follows:

Cd_3(PO_4)_2\rightleftharpoons 3Cd^{2+}+2PO_4^{3-}

                      3s       2s

The expression for solubility constant for this reaction will be:

K_{sp}=[Cd^{2+}]^3[PO_4^{3-}]^2

We are given:

K_{sp}=2.5\times 10^{-33}

Putting values in above equation, we get:

2.5\times 10^{-33}=(3s)^3\times (2s)^2\\\\2.5\times 10^{-33}=108s^5\\\\s=1.18\times 10^{-7}mol/L

Hence, the solubility of Cd_3(PO_4)_2 in water is 1.18\times 10^{-7}mol/L

6 0
3 years ago
A sample of gas (1.9 mol) is in a flask at 21 °C and 697 mm Hg. The flask is opened and more gas is added to the flask. The new
Artyom0805 [142]

Answer: There are now 2.07 moles of gas in the flask.

Explanation:

PV=nRT

P= Pressure of the gas = 697 mmHg = 0.92 atm  (760 mmHg= 1 atm)

V= Volume of gas = volume of container = ?

n = number of moles = 1.9

T = Temperature of the gas = 21°C=(21+273)K= 294 K   (0°C = 273 K)

R= Value of gas constant = 0.0821 Latm\K mol

V=\frac{nRT}{P}=\frac{1.9\times 0.0821 \times 294}{0.92}=49.8L

When more gas is added to the flask. The new pressure is 775 mm Hg and the temperature is now 26 °C, but the volume remains same.Thus again using ideal gas equation to find number of moles.

PV=nRT

P= Pressure of the gas = 775 mmHg = 1.02 atm  (760 mmHg= 1 atm)

V= Volume of gas = volume of container = 49.8 L

n = number of moles = ?

T = Temperature of the gas = 26°C=(26+273)K= 299 K   (0°C = 273 K)

R= Value of gas constant = 0.0821 Latm\K mol

n=\frac{PV}{RT}=\frac{1.02\times 49.8}{0.0821\times 299}=2.07moles

Thus the now the container contains 2.07 moles.

6 0
2 years ago
A sample of gas at 47C and 1.5 pressure occupies a volume of 2.20L. What volume would this gas occupy at 107C and 2.5 pressure?
Brums [2.3K]

Answer:

Explanation:

21

8 0
3 years ago
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