Respuesta :
Answer: The molarity of the stock solution is 4.64 M
Explanation:
To calculate the molarity of the diluted solution, we use the equation:
[tex]M_1V_1=M_2V_2[/tex]
where,
[tex]M_1\text{ and }V_1[/tex] are the molarity and volume of the stock solution
[tex]M_2\text{ and }V_2[/tex] are the molarity and volume of diluted solution
We are given:
[tex]M_1=?M\\V_1=65.5mL\\M_2=0.675M\\V_2=450mL[/tex]
Putting values in above equation, we get:
[tex]M_1\times 65.5=0.675\times 450\\\\M_1=4.64M[/tex]
Hence, the molarity of the stock solution is 4.64 M
Answer:
4.64M
Explanation:
Dilution Problems Worksheet
1. How do you prepare a 250.-ml of a 2.35 M HF dilution from a 15.0 M stock solution?
39.2 mL
2. If 455-ml of 6.0 M HNO3 is used to make a 2.5 L dilution, what is the molarity of the dilution?
1.1 M
3. If 65.5 ml of HCl stock solution is used to make 450.-ml of a 0.675 M HCl dilution, what is the molarity of the stock solution?
4.64 M
4. How do you prepare 500.-ml of a 1.77 M H2SO4 dilution from an 18.0 M H2SO4 stock solution?
Take 49.2-ml of 18.0 M H2SO4 stock solution and pour it into a 500-ml volumetric flask. Fill to the 500-ml line with distilled water to make 1.77M H2SO4 solution.
Extra Molarity Problems for Practice
1. How many moles of LiF would be required to produce a 2.5 M solution with a volume of 1.5 L?
3.75 M
2. How many moles of Sr(NO3)2 would be used in the preparation of 2.50 L of a 3.5 M solution?
8.75 M
3. What is the molarity of a 500-ml solution containing 249 g of KI?
3.00 M
4. How many grams of CaCl2 would be required to produce a 3.5 M solution with a volume of 2.0 L?
777 g
