1. When 5.0 g CaCl2 is dissolved in enough water to make a 0.500 L solution, what is the molarity of ions in solution?
2. How many formula units are in 0.25 mole of Na2O?
3. How many nitrate ions are present in 0.200 mol of Zn(NO3)2?
1)
Molar mass of CaCl2,
MM = 1*MM(Ca) + 2*MM(Cl)
= 1*40.08 + 2*35.45
= 110.98 g/mol
mass(CaCl2)= 5.0 g
use:
number of mol of CaCl2,
n = mass of CaCl2/molar mass of CaCl2
=(5 g)/(1.11*10^2 g/mol)
= 4.505*10^-2 mol
volume , V = 0.5 L
use:
Molarity,
M = number of mol / volume in L
= 4.505*10^-2/0.5
= 9.011*10^-2 M
This is concentration of CaCl2
1 molecule of CaCl2 gives 3 ions which are 1 Ca2+ and 2 Cl-
So,
[ions] = 3*[CaCl2]
= 3*9.011*10^-2 M
= 0.270 M
Answer: 0.270 M
Only 1 question at a time please
1. When 5.0 g CaCl2 is dissolved in enough water to make a 0.500 L solution,...
If 44g of CaCl2 is dissolved in enough water to make 500mL of solution, what will be the molarity M, of the solution? show work
TML 4. Calculate the molarity when 40.0 g of sodium hydroxide is dissolved in enough water to make a 3.0 L solution. M= mol solute 40.09 Nao L soin 37. mi Calculate the more feilver nitrate in 185 ml of a 2.50 M solution.
Solution Worksheet Name 1.12.5 g of NaCl is dissolved in enough water to make 0,683 L of solution: a. What is the molarity of the solution? b. How many moles of Nail are contained in 0.0100 L of the above solution? What volume (L) of this NaCl solution would contain 0.150 moles of NaCl? 2. 255 g of NHCl is dissolved in enough water to make 7500 ml of solution What is the molarity of the solution b. How many...
If 2.63 g Fe(NO3), is dissolved in enough water to make exactly 460 mL of solution, what is the molar concentration of nitrate ion? M of Fe(NO3)3=241.86 g/mole
5.0 g of solid Al(NO3)3 was added to enough water to make a 100.0 mL solution. Al(NO3)3 is very soluble in water. 1. Write out the dissolution reaction that occurs when the solid Al(NO3)3 was added to water. 2. What is the concentration, in Molarity, of Al(NO3)3 once it is dissolved in the water? 3. If 53 mL of water was added to the original Al(NO3)3 solution described above, what is the new concentration in Molarity? 4. What is the...
A 1.04 g sample of KBr is dissolved in water to give 155 mL of solution. This solution is then added to 165 mL of 0.015 M aqueous Pb(NO3)2, in an attempt to remove the toxic lead(II) ions from the solution via precipitation as insoluble PbBr2(s). The precipitation reaction that occurs is: Pb2+ (aq) + 2 Br (aq) ---> PbBr2 (s) At the end of the reaction, what is the concentration (in molarity) of nitrate ions in the solution? Note:...
Question 1 (1 point) A 52.30 g sample of Ba(OH)2 is dissolved in enough water to make 1.20 L of solution. How many milliliters of this solution must be diluted with water in order to make 1.00 L of 0.100 M Ba(OH)2? 62.8 mL 254 mL O 305 ml O 523 mL O 393 mL O Question 2 (1 point) A chemist needs 225 mL of 2.3 M HCl. What volume of 12 M HCl must be dissolved in water...
If 1.25 g Fe(NO3)3 is dissolved in enough water to make exactly 397 mL of solution, what is the molar concentration of nitrate ion?
2. 25.5 g of NHCl is dissolved in enough water to make 750.0 mL of solution What is the molarity of the solution? b. How many moles of ammonium chloride are contained in 237 mL of solution? c. What volume in mL of this solution would contain 0.059 moles of ammonium chloride?
12.5g of glucose (C6H12O6) is dissolved in enough water to make 750.0ml of solution. (molar mass of glucose = 180.16 g) What is the molarity of the solution? How many moles of glucose are contained in 237 ml of the above glucose solution? What volume (L) of this glucose solution would contain 0.079 moles of glucose?