Astudent dissolved 4.00 g of co(no3)2 in enough water to make 100. ml of stock solution. he took 4.00 ml of the stock solution and then diluted it with water to give 275. ml of a final solution. how many grams of no3- ion are there in the final solution?

0.08097 grams of nitrate ions are there in the final solution.

Explanation:

Moles of cobalt(II) nitrate ,n=

Volume of the cobalt(II) nitrate solution, V = 100.0 mL = 0.1 L

Let the molarity of the solution be

A students then takes 4 .00 mL of solution and dilute it to 275 ml.

(molarity after dilution)

(after dilution)

Molarity of the of solution after dilution is 0.002375 M.

1 mol of cobalt(II) nitrate gives 2 moles of nitrate ions. Then 0.002375 M solution of cobalt (II) nitrate will give:

Moles of nitrate ions = n

Volume of the solution = 275 mL = 0.275 L

Molarity of the nitrate ions =

n = 0.001306 mol

Mass of 0.001306 moles of nitrate ions:

0.001306 mol × 62 g/mol= 0.08097 g

0.08097  grams of nitrate ions are there in the final solution.

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.

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