Answer:
1) 0.0625 g.
2) 0.0125 g.
Explanation:
<em>1) A solution of NaOH has a concentration of 25.00% by mass. What mass of NaOH is present in 0.250 g of this solution?</em>
mass% of NaOH = [(mass of NaOH)/(mass of solution)] x 100.
mass% of NaOH = 25.0%, mass of NaOH = ??? g, mass of solution = 0.250 g.
∴ mass of NaOH = (mass% of NaOH)(mass of solution)/100 = (25.0%)(0.250 g)/100 = 0.0625 g.
<em>2) What mass of NaOH must be added to the solution to increase the concentration to 30.00% by mass?</em>
We can use the relation:
mass% of NaOH = [(mass of NaOH)/(mass of solution)] x 100.
mass% of NaOH = 30.0%, mass of NaOH = ??? g, mass of solution = 0.250 g.
∴ mass of NaOH = (mass% of NaOH)(mass of solution)/100 = (30.0%)(0.250 g)/100 = 0.075 g.
∴ The mass of NaOH should be added = 0.075 - 0.0625 = 0.0125 g.
Answer:
What do you need help with
Explanation:
The equation which we are required to complete can be completed as follows;
- AgNO3 + KCl ==> KNO3 + AgCl
<h3>Electrochemical series;</h3>
Most substitution reactions involve displacement of metals and non-metals.
The possibility of a substitution reaction to occur is sometimes dependent on the order of preference of the metals in the activity series.
On this note, In the reaction between AgNO3 and KCl, potassium, K displaces silver, Ag and the products of the reaction are; KNO3 and AgCl
Read More on Electrochemical series;
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