What is the molarity of 2.60l solution that contains 67.3 grams of copper (ii) chloride

0.193 M to the nearest thousandth.

Explanation:

Molar mass of copper (ii) chloride

= 63.546 + 2* 35.45

= 134.446 g.

So in 2.60L of 1  M solution  there is 134.446 * 2.6

= 349.56 g of copper chloride.

So the molarity of our solution is  67.3 / 349.56

= 0.193 M.

percent abundance for cu-63 can be shown as:

63 x + 65 (1-x) = 62.9296

65 - 62.9296 = 2 x

x = 1.035

thus, percent abundance for cu-63 is 1.035

percent abundance for cu-65 can be shown as:

63 x + 65 (1-x) = 64.9278

65 - 64.9278 = 2 x

x = 0.0361

thus, percent abundance for cu-63 is 0.0361

the mass spectrum of cu-63 showing the intense peak as, this isotope is found in nature more abundantly around 92.38 % in comparison to cu-65 which is found 62.58 % naturally