A concentrated solution is 68.4% nitric acid in water and has a density of 1.39

Question

A concentrated solution is 68.4% nitric acid in water and has a density of 1.39 g/mL. How many mL of this nitric solution will completely and exactly react with 143 g of Cu metal? If your answer is within + 2 the last decimal place of one of the choices below, then it is the same number as the choice. Sig figs is going to depend on how many digits you carried in your calculation and how many digits you used for atomic masses. Hint - Balance the reaction first! Cu + NO3^- ----> Cu^+2 + NO
a) 15.1 b) 99.4 c) 2.25 d) 398 e) 768 f) 55.9 g) 22.5

Explanation / Answer

3Cu(s) + 8HNO3(aq) ——> 3Cu(NO3)2(aq) + 2NO(g) + 4H2O(l) actual reaction is above Now moles of Cu metal = 143/ 63.5463 =2.25 moles so HNO3 requirred = (8/3)*2.25 =6 moles 1 mL of solution contains= 1.39g of solution= .684*1.39 g of HNO3 = 0.95 g Also moles of HNO3 per 100 mL = 95/63.01 =1.5076 thus total volume = 100*6/1.5076 =397.98 nearly same as 398 mL thus requirred answer is d)

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