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S_A_V [24]
2 years ago
5

calculate the mass required to prepare 2.5 L of 1.0 M NaOH solution. Given that the molar mass for NaOH is 40 g/mol.

Chemistry
2 answers:
grandymaker [24]2 years ago
4 0

Answer:

100\; \rm g of {\rm NaOH}\; (s) would be required.

Explanation:

The quantity of solute in a solution of concentration c and volume V would be n = c \cdot V.

It is given that volume V = 2.5\; \rm L for the solution in this question. It is also given that the concentration of the \rm NaOH solute in this solution is c = 1.0\; \rm M, which is the equivalent to c = 1.0\; \rm mol \cdot L^{-1}.  

Apply the equation n = c \cdot V to find the quantity of \rm NaOH in this solution:

\begin{aligned}n &= c \cdot V \\ &= 1.0\; \rm mol \cdot L^{-1} \times 2.5\; \rm L \\ &= 2.5\; \rm mol\end{aligned}.

Multiply the quantity n of \rm NaOH in this solution with the formula mass M of {\rm NaOH}\! to find the corresponding mass:

\begin{aligned}m &= n \cdot M \\ &= 2.5\; \rm mol \times 40\; \rm g \cdot mol^{-1} \\ &= 100\; \rm g\end{aligned}.

Thus, this solution would contain 100\; \rm g of {\rm NaOH}.

It would thus take 100\; \rm g of {\rm NaOH} to prepare this solution.

Helen [10]2 years ago
3 0

Answer:

The required mass to prepare 2.5 L of 1.0 M NaOH solution is 100 g

Explanation:

We do this by preparing the equation:

Mass = concentration (mol/L) x volume (L) x Molar mass

Mass = 1.0 M x 2.5 L x 40 g/mol

Mass = 100 g

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4 0
3 years ago
A chemist must prepare 300.0mL of nitric acid solution with a pH of 0.70 at 25°C. He will do this in three steps: Fill a 300.0mL
d1i1m1o1n [39]

<u>Answer:</u> The volume of concentrated solution required is 9.95 mL

<u>Explanation:</u>

To calculate the pH of the solution, we use the equation:

pH=-\log[H^+]

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Putting values in above equation, we get:

0.70=-\log[H^+]

[H^+]=10^{-0.70}=0.199M

1 mole of nitric acid produces 1 mole of hydrogen ions and 1 mole of nitrate ions.

Molarity of nitric acid = 0.199 M

To calculate the volume of the concentrated solution, we use the equation:

M_1V_1=M_2V_2

where,

M_1\text{ and }V_1 are the molarity and volume of the concentrated nitric acid solution

M_2\text{ and }V_2 are the molarity and volume of diluted nitric acid solution

We are given:

M_1=7.0M\\V_1=?mL\\M_2=0.199M\\V_2=350mL

Putting values in above equation, we get:

7.0\times V_1=0.199\times 350.0\\\\V_1=\frac{0.199\times 350}{7.0}=9.95mL

Hence, the volume of concentrated solution required is 9.95 mL

6 0
2 years ago
What is the mass of 2.5 mol of ca, which has a molar mass of g/mol
swat32
Atomic mass Ca = 40 a.m.u

1 mole Ca ----------- 40 g
2.5 mols Ca -------- ( mass Ca )

Mass Ca = 2.5 x 40 / 1

Mass Ca = 100 / 1

= 100 g of Ca

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