Explanation:
It is known that molarity is the number of moles present in a liter of solution.
Mathematically, Molarity =
Hence, calculate the molarity of given solution as follows.
Molarity of citric acid =
=
= 0.173 M
As citric acid is a triprotic acid so, upon dissociation it gives three hydrogen ions.
Normality = Molarity × no. of hydrogen or hydroxide ions
= 0.173 × 3
= 0.519 N
Thus, we can conclude that molarity of given solution is 0.173 and its normality is 0.519 N.
Answer:- 2.39 mL are required.
Solution:- It's a dilution problem and to solve this type of problems we use the dilution equation:
Where, and
are molarities of concentrated and diluted solutions and
and
are their respective volumes.
= 1.10M
= 5.00mM = 0.005M (since, mM stands for milli molar and M stands for molar. 1M = 1000mM)
= ?
= 525 mL
Let's plug in the given values in the formula:
So, 2.39 mL of 1.10M are needed to make 525 mL of 5.00mM solution.
Answer:
32g
Explanation:
potassium nitrate has solubility of about 67g per 100g of water at 40°C, which means that potassium nitrate solution will contain 67g of dissolved salt for every 100g of water.
since at this temperature, our solution contains 35g of potassium nitrate 100g of water. The solution will be unsaturated because of the less potassium nitrate.
to make saturated solution,
mass of potassuim nitrate = 67g - 35g
= 32g
which means dissolving another 32g of potassium nitrate in solution at 40 °C will make saturated solution.
