The question is incomplete, here is the complete question:
A chemist prepares a solution of copper(II) sulfate 
by measuring out 69.2 g of copper(II) sulfate into a 400. mL volumetric flask and filling the flask to the mark with water.
Calculate the concentration in mol/L of the chemist's copper(II) sulfate solution. Round your answer to 3 significant digits.
<u>Answer:</u> The molarity of copper (II) sulfate solution is 1.08 mol/L
<u>Explanation:</u>
To calculate the molarity of solution, we use the equation:
We are given:
Given mass of copper (II) sulfate = 69.2 g
Molar mass of copper (II) sulfate = 159.6 g/mol
Volume of solution = 400. mL
Putting values in above equation, we get:
Hence, the molarity of copper (II) sulfate solution is 1.08 mol/L
What do you need help with?
Answer:
ΔH=15000
J = 15KJ
Explanation:
In this exercise you have find the enthalpy of reaction this is the difference between enthalpy of reactans and products,
For the following equation
H2A(aq) + 2 BOH(aq) → B2A(aq) + 2 H2O(l)
We know that 0.20 moles of BOH reacted with excess amount of H2A solution and 1500. J
so,
(2mol/0,2mol)*1500J=15000J
for de reactions exothermics tha enthalpy is negative so:
ΔH=15000
J = 15KJ
I don't know if that's the whole question or if you forgot the answer choices, but
Copper and Fluorine are one of the ones ( I know of) that are likely to form Ionic bonds.
Hope this helps. :)
Yo sup??
The answer to your question is option c ie
c.9
the rest 12 are under non essential as they are produced by our body itself
Hope this helps.
