<span>1 mole of carbon has 12 grams, so 23 moles equals 276 grams of carbon
23 x 12 = 276 grams of carbon</span>
The aluminum sulfate stock solution should the chemist pour out is 219.8 ml
Complete Question
A chemist must prepare 400 mL of 1.00M aqueous aluminum sulfate working solution. He'll do this by pouring out 1.82 mol/L aqueous aluminum sulfate stock solution into a graduated cylinder and diluting it with distilled water. How many mL of the aluminum sulfate stock solution should the chemist pour out?
The aluminum sulfate stock solution should the chemist pour out is 219.8 ml
Given:
V1 = 400ml, M1 = 1 M, V2 = ?, M2 = 1.82 M
Hence, the relation between molarity and volume is as follows.
M1V1 = M2V2
1.00M x 400ml = 1.82 x V2
V₂ = 219.8 ml
Thus, we can conclude that 219.8 ml of the aluminum sulfate stock solution should the chemist pour out.
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Answer:
1.Sn
2.Sn
Explanation:
1. Sn oxidizes to Sn2+
The oxidation number increases from 0 to +2 by removing 2 electrons
Sn ----> Sn²+ & 2e
(Oxidation is the removal of electrons)
2. In a galvanic cell, oxidation takes place at the anode, hence tin is the anode