(b) If the natural abundance of Ag-107 is 51.84%, what is the natural abundance of Ag-109?
%
(c) If the mass of Ag-107 is 106.905, what is the mass of Ag-109?
amu
I really need help. Can u say the answer then explain how you got it?
Thanks:)
Oops I just need c
106.905(0.5184) + massAg109(1-0.5184) = mass Ag from periodic table.
Solve for the only unknown which is mass Ag 109.
Remember the isotopes are averaged to obtain the atomic mass found in the periodic table.
THE FOLLOWING SOLUTIONS AREMIXED TOGETHER: 121mL OF 1.54 M AgNO3 AND 45mL OF 1.07 M K2SO4
CALCULATE THE MOLAR CONCENTRATION OF Ag+ IONS IN THE FINAL SOLUTION
Certainly! Let's solve both parts step by step.
(b) The natural abundance of Ag-107 is given as 51.84%. To find the natural abundance of Ag-109, we need to consider that the sum of the abundances of all isotopes of an element is 100%.
Since Ag-107 and Ag-109 are the only two isotopes mentioned, we can set up the following equation:
Abundance of Ag-107 + Abundance of Ag-109 = 100%
Given that the natural abundance of Ag-107 is 51.84%, we can substitute this into the equation:
51.84% + Abundance of Ag-109 = 100%
To solve for the abundance of Ag-109, we subtract 51.84% from both sides of the equation:
Abundance of Ag-109 = 100% - 51.84%
= 48.16%
So, the natural abundance of Ag-109 is 48.16%.
(c) To find the mass of Ag-109, we first need to know the atomic mass of Ag-107. According to the question, the atomic mass of Ag-107 is given as 106.905 amu.
Ag-107 is the more abundant isotope, so its mass should be closer to the average atomic mass of silver.
We can set up an equation to determine this:
(Abundance of Ag-107 * Mass of Ag-107) + (Abundance of Ag-109 * Mass of Ag-109) = Average atomic mass
Substituting the given information, we have:
(51.84% * 106.905 amu) + (48.16% * Mass of Ag-109) = Average atomic mass
We know that the average atomic mass of silver is typically 107.87 amu, so we can substitute this value into the equation:
(51.84% * 106.905 amu) + (48.16% * Mass of Ag-109) = 107.87 amu
Now, we need to solve for the mass of Ag-109. First, multiply the abundance of Ag-109 by its mass:
48.16% * Mass of Ag-109 = 107.87 amu - (51.84% * 106.905 amu)
Next, divide both sides of the equation by 48.16%:
Mass of Ag-109 = (107.87 amu - (51.84% * 106.905 amu)) / 48.16%
Calculating this out, we get:
Mass of Ag-109 = (107.87 amu - (0.5184 * 106.905 amu)) / 0.4816
Mass of Ag-109 = (107.87 amu - 55.391992 amu) / 0.4816
Mass of Ag-109 = 52.478008 amu / 0.4816
Mass of Ag-109 ≈ 108.879 amu
Therefore, the approximate mass of Ag-109 is 108.879 amu.