How many milliliters of 0.200M #NaOH# solution are needed to react with 22.0 mL of a 0.490 M #NiCl_2# solution?
There are
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To find the volume of the NaOH solution needed to react with the NiCl2 solution, we can use the stoichiometry of the reaction. The balanced chemical equation for the reaction between NaOH and NiCl2 is:
2NaOH + NiCl2 → Ni(OH)2 + 2NaCl
From the equation, we can see that 2 moles of NaOH react with 1 mole of NiCl2. Therefore, we can use the formula:
( \text{Volume}{\text{NaOH}} \times \text{Molarity}{\text{NaOH}} \times \frac{2}{1} = \text{Volume}_{\text{NiCl}2} \times \text{Molarity}{\text{NiCl}_2} \times \frac{1}{1} )
Plugging in the given values:
( \text{Volume}_{\text{NaOH}} \times 0.200 , \text{M} \times \frac{2}{1} = 22.0 , \text{mL} \times 0.490 , \text{M} \times \frac{1}{1} )
Solving for ( \text{Volume}_{\text{NaOH}} ):
( \text{Volume}_{\text{NaOH}} = \frac{22.0 , \text{mL} \times 0.490 , \text{M}}{0.200 , \text{M} \times 2} )
( \text{Volume}_{\text{NaOH}} = 54.45 , \text{mL} )
So, 54.45 milliliters of the 0.200 M NaOH solution are needed to react with 22.0 mL of the 0.490 M NiCl2 solution.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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