A chemistry student needs 90.0mL of carbon tetrachloride for an experiment. By consulting the CRC Handbook of Chemistry and Phys
1 answer:
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We know that 1 mole of anything has a volume of 22.4 liters.
And 1 mole of N2 gas has a weight of 28 grams.
Comparing them , we get the answer as 5.31
Answer:
a) 5,3176x10⁻⁴ moles
b) 6,85x10⁻⁴ moles
c) The appropriate formula to calculate is Henderson-Hasselbalch.
d) pH = 4,86. Acidic solution but slighty
Explanation:
a) moles of acetic acid:
9,20x10⁻³L × 57,8x10⁻³M = <em>5,3176x10⁻⁴ moles</em>
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b) moles of sodium acetate:
56,2x10⁻³g ÷ 82,0 g/mole = <em>6,85x10⁻⁴ moles</em>
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c) The appropriate formula to calculate is Henderson-Hasselbalch:
pH= pka + log₁₀
d) pH= 4,75 + log₁₀
<em>pH = 4,86</em>
<em>3 < pH < 7→ Acidic solution but slighty</em>
I hope it helps!
Answer:
3.72 mol Hg
General Formulas and Concepts:
<u>Chemistry - Atomic Structure</u>
- Reading a Periodic Table
- Using Dimensional Analysis
- Density = Mass over Volume
Explanation:
<u>Step 1: Define</u>
D = 13.6 g/mL
54.8 mL Hg
<u>Step 2: Identify Conversions</u>
Molar Mass of Hg - 200.59 g/mol
<u>Step 3: Find</u>
13.6 g/mL = x g / 54.8 mL
x = 745.28 g Hg
<u>Step 4: Convert</u>
<u /> = 3.71544 mol Hg
<u>Step 5: Check</u>
<em>We are given 3 sig figs. Follow sig fig rules and round.</em>
3.71544 mol Hg ≈ 3.72 mol Hg