Which barium nitrate solution requires the greatest moles of solute?
1 answer:
Answer:
The answer to your question is: letter E, 1.77 L of 1.55 M Ba(NO3)2
Explanation:
Formula
Molarity =
moles = Molarity x volume (L)
a. 2.58 L of 0.0250 M Ba(NO3)2
moles = (0.025) (2.58)
moles = 0.065 M
b. 19.23 mL of 8.5 × 10−2 M Ba(NO3)2
moles = (8.5 x 10 ⁻²) (0.01923)
moles = 0.0016
c. No right answer.
d. 26.20 mL of 2.21 M Ba(NO3)2
moles = (2.21)(0.0262)
moles = 0.058
e. 1.77 L of 1.55 M Ba(NO3)2
moles = (1.55)(1.77)
moles = 2.74 This solution needs the greatest concentration of
Ba(NO₃)₂
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Answer:
See explanation
Explanation:
Hello there!
In this case, since the the concentrations are not given, and not even the Ksp, we can solve this problem by setting up the chemical equation, the equilibrium constant expression and the ICE table only:
Next, the equilibrium expression according to the produced aqueous species as the solid silver chloride is not involved in there:
And therefore, the ICE table, in which x stands for the molar solubility of the silver chloride:
I - 0 0
C - +x +x
E - x x
Which leads to the following modified equilibrium expression:
Unfortunately, values were not given, and they cannot be arbitrarily assigned or assumed.
Regards!
Answer: The empirical formula for the given compound is
Explanation:
The chemical equation for the combustion of compound having carbon and hydrogen follows:
where, 'x' and 'y' are the subscripts of carbon and hydrogen respectively.
We are given:
Mass of
We know that:
Molar mass of carbon dioxide = 44 g/mol
For calculating the mass of carbon:
In 44 g of carbon dioxide, 12 g of carbon is contained.
So, in 22.0 g of carbon dioxide, of carbon will be contained.
For calculating the mass of hydrogen:
Mass of hydrogen = Mass of sample - Mass of carbon
Mass of hydrogen = 7.0 g - 6 g
Mass of hydrogen = 1.0 g
To formulate the empirical formula, we need to follow some steps:
Step 1: Converting the given masses into moles.
Moles of Carbon =
Moles of Hydrogen =
Step 2: Calculating the mole ratio of the given elements.
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.5 moles.
For Carbon =
For Hydrogen =
Step 3: Taking the mole ratio as their subscripts.
The ratio of Fe : C : H = 1 : 2
Hence, the empirical formula for the given compound is