10 down: Particle with no charge
Answer: Neutron
Answer:
[MgSO₄] = 890 mM/L
Explanation:
In order to determine molarity we need to determine the moles of solute that are in 1L of solution.
Solute: MgSO₄ (10.7 g)
Solvent: water
Solution: 100 mL as volume. (100 mL . 1L / 1000mL) = 0.1L
We convert the solute's mass to moles → 10.7 g / 120.36 g/mol = 0.089 moles
Molarity (mol/L) → 0.089 mol/0.1L = 0.89 M
In order to calculate M to mM/L, we make this conversion:
0.89 mol . 1000 mmoles/ 1 mol = 890 mmoles
Answer:
506.912 L
Explanation:
From the question given above, the following data were obtained:
Number of mole of O₂ = 22.63 moles
Volume of O₂ =?
Recall:
1 mole of a gas occupy 22.4 L at STP.
With the above information, we obtained the volume occupied by 22.63 moles of O₂ as follow:
1 mole of O₂ occupied 22.4 L at STP.
Therefore, 22.63 moles of O₂ will occupy = 22.63 × 22.4 = 506.912 L at STP.
Thus, 22.63 moles of O₂ is equivalent to 506.912 L.
<h2>Question↷</h2>
Which of these solutions is the most basic?
[OH-] = 4.3 x 10-9 M
[OH-] = 2.8 x 10-11 M
[OH-] = 6.7 x 10-10 M
[OH-] = 1.0 x 10-5 M
<h2>Answer↷</h2>
- <u>[OH-] = 1.0 x 10-5 M</u> ✓
<h2>Solution↷</h2>
[OH-] = 4.3 x 10-9 M
- [OH-] = 4.3 x 10^-9 M
- pOH = - log [OH^1-]
- pOH = - log [4.3 x 10^-9]
- pOH = 8.36
- pH = 14- 8.36
- pH = 5.64
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[OH-] = 2.8 x 10-11 M
- [OH-] = 2.8 x 10^-11 M
- pOH = - log [OH^1-]
- pOH = - log [2.8 x 10^-11 ]
- pOH = 10.55
- pH = 14-10.55
- pH = 3.45
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[OH-] = 6.7 x 10-10 M
- [OH-] = 6.7 x 10^-10 M
- pOH = - log [OH^1-]
- pOH = - log [6.7 x 10^-10]
- pOH = 9.17
- pH = 14-9.17
- pH = 4.83
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[OH-] = 1.0 x 10-5 M
- [OH-] = 1.0 x 10-5 M
- pOH = - log [OH^1-]
- pOH = - log [1.0 x 10^-5 ]
- pOH = 5
- pH = 14-5
- pH = 9
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we know that , the solution with <u>pH > 7</u> is termed as basic and more the pH ,more the basicity, hence ,the solution with the highest pH would be the strongest base out of these all which is
<u>[OH-] = 1.0 x 10-5 M</u> with pH = 9
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