How many milliliters of .200 M NaOH solutions are needed to react with 40.0 mL of a 0.340 M NiCl2 solution?
Equation: NiCl2(aq) + 2NaOH(aq) --> Ni(OH)2(s) +2NaCl(aq)
mols NiCl2 = M x L = ?
mols NaOH = 2 x mols NiCl2.
M NaOH = mols NaOH/L NaOH. You know mols and M NaOH, solve for L and convert to mL.
1360 mL
To determine the volume of 0.200 M NaOH solution needed to react with 40.0 mL of 0.340 M NiCl2 solution, we can use the stoichiometry and the concept of molarity.
First, let's write down the balanced chemical equation:
NiCl2(aq) + 2NaOH(aq) → Ni(OH)2(s) + 2NaCl(aq)
From the equation, we can see that one mole of NiCl2 reacts with two moles of NaOH. This means the mole ratio of NiCl2 to NaOH is 1:2.
Now, let's find the moles of NiCl2 in the given volume of solution. To do this, we can use the formula:
moles of solute = concentration of solution (in moles/L) × volume of solution (in liters)
moles of NiCl2 = 0.340 M × 0.040 L = 0.0136 moles
According to the stoichiometry, since the mole ratio of NiCl2 to NaOH is 1:2, the moles of NaOH needed will be twice the moles of NiCl2:
moles of NaOH = 2 × 0.0136 moles = 0.0272 moles
Finally, we can use the concentration of the NaOH solution to determine the volume needed. Rearranging the formula for moles of solute, we get:
volume of solution (in liters) = moles of solute / concentration of solution (in moles/L)
volume of NaOH = 0.0272 moles / 0.200 M = 0.136 L
However, we need the volume in milliliters as given in the question. To convert liters to milliliters, we multiply by 1000:
volume of NaOH = 0.136 L × 1000 mL/L = 136 mL
Therefore, 136 milliliters of 0.200 M NaOH solution are needed to react with 40.0 mL of 0.340 M NiCl2 solution.