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Answer:
We have to add 17.2 grams of aluminium bromide
Explanation:
Step 1: Data given
Molarity of the aluminum bromide solution = 0.215 M
Volume = 300 mL = 0.300 L
Molar mass aluminium bromide = 266.69 g/mol
Step 2: Calculate moles Aluminium bromide
moles AlBr3 = volume * molarity
Moles AlBr3 = 0.300 L * 0.215 M
Moles AlBR3 = 0.0645 moles
Step 3: Calculate mass aluminium bromide
Mass aluminium bromide = moles AlBr3 * molar mass AlBr3
Mass aluminium bromide = 0.0645 moles * 266.69 g/mol
Mass aluminium bromide = 17.2 grams
We have to add 17.2 grams of aluminium bromide
Answer:
2,53x10⁻³ moles of NaOH
Explanation:
The reactions of a diprotic acid with NaOH are:
H₂X + NaOH → HX⁻ + H₂O + Na⁺
HX⁻ + NaOH → X²⁻ + H₂O + Na⁺
Where the complete first reaction gives the first equivalence point and the complete second reaction gives the second equivalence point.
The total volume spent of NaOH to reach the second equivalence point is:
7,00mL + 14,07mL = 21,07 mL = <em>0,02107L</em>
As molar concentration of NaOH is 0,120M, the moles used to reach the second equivalence point are:
0,02107L×(0,120mol/L) = <em>2,53x10⁻³ moles of NaOH</em>
I hope it helps!
The number of valence electrons for each molecule or ion is shown beneath the structure. Remember hydrogen will not have more than two electrons. This hydrogen is part of a covalent bond (sharing two electrons). A double bond here would cause hydrogen to share four electrons with phosphorus.
