Problem: If the following solutions are mixed, is the resulting solution acidic, basic, or neutral?125.0 mL of 0.100 M HNO3 and 80.0 mL of 0.0750 M Ca(OH)2

FREE Expert Solution

Step 1: Calculate the initial amount (in moles) of the HNO3 and Ca(OH)2 

Recall:

molarity (M)=molL

moles HNO3=0.100 mol HNO3L 125.0 mL x 10-3 L1 mL

moles HNO3 = 0.0125 mol HNO3

moles Ca(OH)2=0.0750 mol Ca(OH)2L80.0 mL x 10-3 L1 mL

moles Ca(OH)2 = 0.006 mol Ca(OH)2


The amount of HNO3 is greater than Ca(OH)2, therefore there will be HNO3 left after the reaction


Step 2: Calculate the amount of HNO3 reacted

Balanced reaction:                 2HNO3 + Ca(OH)2 → 2 H2O(l) + Ca(NO3)2(aq)

2 mole of HNO3 reacts with 1 mole of Ca(OH)2:
mol of HNO3 reacted = mol Ca(OH)2 reacted÷2

moles HNO3 reacted = 0.0023 mol HNO3


Step 3: Calculate the amount of HNO3 left after the reaction

moles HNO3 left = moles HNO3 (initial) – moles HNO3 (reacted)

moles HNO3 left = 0.0125 mol HNO3 - 0.003 mol HNO3

moles HNO3 left 0.0095 mol HNO3


Step 4: Calculate the concentration of HNO3 left in the solution

molarity (M)=molL


final volume of solution=volume HNO3+volumeCa(OH)2 final volume of solution=125.0 mL x 10-3 L1 mL+80.0 mL x 10-3 L1 mLfinal volume of solution=0.125 L+0.080 L

Final Volume of solution = 0.205 L


molarity=0.0095 mol HNO30.205 Lmolarity=0.0463 mol HNO3L

molarity = 0.0463 M HNO3

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Problem Details

If the following solutions are mixed, is the resulting solution acidic, basic, or neutral?

125.0 mL of 0.100 M HNO3 and 80.0 mL of 0.0750 M Ca(OH)2

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