Answer:
3.816 × 10⁻³ M
Explanation:
<em>A stock solution of Cu²⁺(aq) was prepared by placing 0.8875 g of solid Cu(NO₃)₂∙2.5H₂O in a 100.0-mL volumetric flask and diluting to the mark with water. What is the concentration (in M) of Cu²⁺(aq)in the stock solution?</em>
<em />
We can establish the following relations:
- The molar mass of Cu(NO₃)₂∙2.5H₂O is 232.59 g/mol.
- 1 mole of Cu(NO₃)₂∙2.5H₂O contains 1 mole of Cu²⁺.
The moles of Cu²⁺ in 0.8875 g of Cu(NO₃)₂∙2.5H₂O are:
The molarity of Cu²⁺ is:
<span>3) which is an example of a physical change
</span><span>a) grinding pepper</span>
According to my calculations, C should be correct as 1.00 mole of any substance is 6.022 x 10^23 which is known as Avogadro's number.
Answer:
Volume in L = 0.50 L
Explanation:
Given data:
Molarity of solution = 0.1850 M
Mass of BaCl₂ = 19.30 g
Volume of solution = ?
Solution:
First of all we will calculate the number of moles of solute:
Number of moles = mass/molar mass
Molar mass of BaCl₂ = 208.23 g/mol
Number of moles = 19.30 g / 208.23 g/mol
Number of moles = 0.093 mol
Volume of solution:
Molarity = number of moles of solute / volume of solution in L
0.1850 M = 0.093 mol / Volume in L
Volume in L = 0.093 mol / 0.1850 M (M= mol/L)
Volume in L = 0.50 L
I would say “ends with -ic” , “starts with hydro”,
