Question options:
A) K2SO4
B) FeCl₃
C) NaOH
D) NH₃
E) KCl
Answer:
D. NH₃
Explanation:
K2SO4 = 2 K+ + SO42-
[K+]= 2 x 1.0 = 2.0 M ; [SO42-] = 1.0 M
total concentrations of ions = 2.0 + 1.0 = <em>3.0 M</em>
FeCl3 = Fe3+ + 3Cl-
[Fe3+] = 1.0 M ; [Cl-] = 3 x 1.0 = 3.0
total concentration ions = 1.0 + 3.0 =<em> 4.0 M</em>
NaOH = Na+ + OH-
[Na+] = [OH-] = 1.0 M
total concentration ions = 1.0 + 1.0 = <em>2.0 M</em>
<u>NH3 is a weak acid so the concentration of NH4+ and OH- </u><u><em>< 2.0</em></u>
KCl = K+ + Cl-
[K+] = [Cl-] = 1.0 M
total concentration ions = 1.0 + 1.0 =<em> 2.0 M</em>
Answer:
The formula of the original halide is SrCl₂.
Explanation:
- The balanced equation of this reaction is:
SrX₂ + H₂SO₄ → SrSO₄ + 2 HX, where X is the halide.
- From the equation stichiometry, 1.0 mole of strontium halide will result in 1.0 mole of SrSO₄.
- The number of moles of SrSO₄ <em>(n = mass/molar mass) </em>= (0.755 g) / (183.68 g/mole) = 4.11 x 10⁻³ mole.
- The number of moles of SrX are 4.11 x 10⁻³ moles from the stichiometry of the balanced equation.
- n = mass / molar mass, n = 4.11 x 10⁻³ moles and mass = 0.652 g.
- The molar mass of SrX₂ = mass / n = (0.652) / (4.11 x 10⁻³ moles) = 158.62 g/mole.
- The molar mass of SrX₂ (158.62 g/mole) = Atomic mass of Sr (87.62 g/mole) + (2 x Atomic mass of halide X).
- The atomic mass of halide X = (158.62 g/mole) - (87.62 g/mole) / 2 = 71 / 2 g/mole = 35.5 g/mole.
- This is the atomic mass of Cl.
- <em>So, the formula of the original halide is SrCl₂</em>.
Kc= (nh4)
--------
(nh3) + (h2o)
Answer:
moles of calcium hydroxide= 21.75 mol
a) 43.5 mol
b) 7.25 mol
Explanation:
Please see the attached picture for the full solution.
Combination
Hope this helps :)
