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polet [3.4K]
3 years ago
13

Aqueous solutions of barium nitrate and potassium phosphate are mixed. What is the precipitate and how many molecules are formed

?
Chemistry
2 answers:
kykrilka [37]3 years ago
8 0

Aqueous solutions of barium nitrate and potassium phosphate are mixed. What is the precipitate and how many molecules are formed?

Barium nitrate has a chemical symbol of Ba(NO3)2 and potassium phosphate has a chemical symbol K2PO4. The reaction between these two is a double replacement reaction yielding barium phosphate and potassium nitrate.

The chemical equation representing the reaction is,

            Ba(NO3)2 + K2PO4 à KNO3 + BaPO4

Anna007 [38]3 years ago
6 0

Answer: The precipitate is Ba_3(PO_4)_2 and 1 molecule of Barium phosphate and 6 molecules of Potassium nitrate is formed.

Explanation: We are given Barium nitrate and Potassium phosphate , that will lead to the formation of Barium phosphate and Potassium nitrate.

As we know that these solutions are present in water, therefore we will obtain Barium phosphate as a precipitate because Barium phosphate is insoluble in water and Potassium nitrate is soluble in water. Thus the reaction is

Ba(NO_3)_2(aq.)+K_3PO_4(aq.)\rightarrow Ba_3(PO_4)_2(ppt.)+KNO_3(aq.)

To know how many molecules are formed at the end, we need to balance the above equation.

Balancing the equation, we get:

3Ba(NO_3)_2(aq.)+2K_3PO_4(aq.)\rightarrow Ba_3(PO_4)_2(ppt.)+6KNO_3(aq.)

Thus, we get 1 molecule of Barium phosphate as a precipitate and 6 molecules of Potassium nitrate which is easily soluble in water.


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A saturated solution of baso4 has a concentration of 0.5mol/l. a 55ml sample is taken by you. what is the mass of baso4 in the s
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6.4 g BaSO₄

Explanation:

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Molarity (mol/L) = moles / volume (L)

(Step 1)

55 mL / 1,000 = 0.055 L

Molarity = moles / volume                             <----- Molarity ratio

0.5 (mol/L) = moles / 0.055 L                        <----- Insert values

0.0275 = moles                                             <----- Multiply both sides by 0.055

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Molar Mass (BaSO₄): 137.33 g/mol + 32.065 g/mol + 4(15.998 g/mol)

Molar Mass (BaSO₄): 233.387 g/mol

0.0275 moles BaSO₄          233.387 g
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