Question

What mass of NaCl is needed to produce a 500 g of a 6.40% M/M solution?

What is the concentration, in g/100 mL, of a solution made by dissolving 123.2 g of phosphoric acid in 50.0 mL of solution?

How much water is needed to produce a 0.68 M solution of copper (I) carbonate, if 3.58 g is used?

What mass of carbon dioxide would you add to 1 500 L of water in order to make a 325 ppm solution?

What is the concentration of a solution made by diluting 14.0 mL of a 4.20 M Na2CO3 to 86.0 mL?

To what volume should 58.3 mL of a 1.4 M KCl solution be diluted to produce a 0.45 M solution?

What volume of a 6.0 M NaOH solution is needed to produce 3.0 L of a 0.1 M solution?

What mass of aluminum nitrate do you need to prepare 3.58 L of a 1.77 M solution?

Zinc iodide is dissolved in 2.5 L of water to make a solution. 1 L of this solution is then diluted to make 12.0 L of a 0.5 M solution. What mass of zinc iodide was added to make the original solution?

Explain the steps you would follow to make 500 mL of a 0.3 M solution of sucrose (C12H22O11) in the lab

Answer 1

1. $\%m/m \ of \ a solution=\dfrac{solute \ mass }{solution\ mass}×100$

$6.4=\dfrac{solute\ mass}{500}×100$

Mass of $NaCl\ required=32g$

2. Concentration of a solution$=\dfrac{ 123.2g}{50ml}=\dfrac{x}{100}$

$=123.2*100=12320g/ml$

$x=242.6g$

3.

Molarity$=\dfrac{moles}{ volume(L)}$

Moles of copper (i) carbonate $=\dfrac{mass}{ molar mass}$

$=\dfrac{3.58}{187}=0.019$

$0.68=\dfrac{0.019}{L}$

$L=281.54mL$

4.

$1ppm=1mg/L\ in\ aq\ solutions\newline For 325ppm=325mg/L\newline Therefore,\newline 1500L*325mg=487/500mg \ Mass=488g\ of\ CO_2 \ required$

5.

$C1V1=C2V2\newline C1*86=4.26*14 \newline C1=0.68\newline =0.68M$

6.

$\dfrac{58.3ml*0.4M}{0.45M}=181mL$

7.

$M1V1=M2V2\newline 6.0*V1=0.1*3.0\newline V1=\dfrac{0.1*3.0}{6.0}$

$V1=0.05L \ of\ NaOH\ is\ needed$