Answer : The concentrations of hydroxide and hydronium ions in a solution with a pH of 10.2 are, and respectively.
Explanation : Given,
pH = 10.2
pH : It is defined as the negative logarithm of the hydrogen ion concentration.
First we have to calculate the hydrogen ion concentration
Now put the value of pH in this formula, we get the hydrogen ion concentration.
Now we have to calculate the pOH of the solution.
Now put the value of pH, we get the value of pOH.
Now we have to calculate the hydroxide ion concentration
Now put the value of pOH in this formula, we get the hydroxide ion concentration.
Therefore, the concentrations of hydroxide and hydronium ions in a solution with a pH of 10.2 are, and respectively.
Answer:
Explanation:
Molarity is found by dividing the moles of solute by liters of solution.
We know the molarity is 1.2 M (mol\liter) and there are 2.3 liters of solution. Substitute the known values into the formula.
Since we are solving for x, we must isolate the variable. It is being divided by 2.3 and the inverse of division is multiplication. Multiply both sides by 2.3 liters.
In a solution with a molarity of 1.2 and 2.3 liters of solution, there are 2.76 moles.
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Answer:
See the attached file for the structure
Explanation:
See the attached file for the explanation
MMn = 54.94g/mol
MO2 = 2(16) = 32g/mol
MH = 1g/mol
MCl = 35.45g/mol
Molar Mass of MnO2:
54.94
+
2
(
16
)
=
86.94
Molar Mass of HCl:
1
+
35.45
=
36.45
Looking at the equation, we need a 4:1 ratio of HCl to MnO2 to make the reaction work, let's see if we have four times as much of the HCl.
Mols of MnO2:
42.7
86.94
=
0.49
Mols of HCl:
47.1
36.45
=
1.29
As we can see, we have less than the amount of HCl we need for all of the MnO2 to react, therefore the HCl is the limiting reactant.
For the theoretical yield of Cl2, we need to determine how many mols will be produced. As we can see by the equation, four mols of HCl make one mol of Cl2.
Molar Mass of Cl2:
35.45
⋅
2
=
70.9
Since we have 1.29mol of HCl, and we know it is the limiting reactant:
Mols of Cl2
1.29
4
=
0.323
Mass of Cl2 (Theoretical yield)
0.323
⋅
70.9
=
22.9
To calculate the actual yield, we multiply the theoretical yield by the final percentage:
22.9
⋅
0.791
=
18.11
Therefore, the actual yield of chlorine is 18.11