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Elden [556K]
3 years ago
8

Which is a strong base? HCl NaOH NH3 H3CO3

Chemistry
1 answer:
STatiana [176]3 years ago
6 0

Answer:

The answer is B: NaOH :3

Explanation:

Hope this helped :D

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Oxidation number ofAl2S12O7
Savatey [412]

Answer:

-2? if wrong im sorry please tell me what I did that was incorrect ty  Explanation:

6 0
2 years ago
Unknown element x is a metal that ionically bonds to sulfur.is the formula, x3s feasible? why or why not?a)it is feasible. the t
nasty-shy [4]
The correct answer is:
d) No, it is not feasible. three metallic ions cannot provide the exact number of electrons that one sulfur needs for the ionic bond.
Because Sulfur is divalent so it need to gain 2 electrons from metal so if we have 3 metals they can't provide only two electrons only.
8 0
3 years ago
Read 2 more answers
You have 50 ml of a complex mixture of weak acids that contains some HF (pKa = 3.18) and some HCN (pKa = 9.21). Which is larger,
bonufazy [111]

Answer:

\frac{[F^{-}]}{[HF]} is larger

Explanation:

pK_{a}=-logK_{a} , where K_{a} is the acid dissociation constant.

For a monoprotic acid e.g. HA, K_{a}=\frac{[H^{+}][A^{-}]}{[HA]} and \frac{[A^{-}]}{[HA]}=\frac{K_{a}}{[H^{+}]}

So, clearly, higher the K_{a} value , lower will the the pK_{a}

In this mixture, at equilibrium, [H^{+}] will be constant.

K_{a} of HF is grater than K_{a} of HCN

Hence, (\frac{F^{-}}{[HF]}=\frac{K_{a}(HF)}{[H^{+}]})>(\frac{CN^{-}}{[HCN]}=\frac{K_{a}(HCN)}{[H^{+}]})

So, \frac{[F^{-}]}{[HF]} is larger

5 0
3 years ago
Determine the molarity of a solution with a volume of 435. mL and 0.550 mol of solute dissolved.
lora16 [44]

Answer:

M = 1.26

Explanation:

Molarity = mole of solution/liters of solution
435mL/1000 = .435L
Plugging in the numbers into the formula, we get:
Molarity = .550 mol/.435L = 1.26 M

8 0
2 years ago
I need help with these
nikklg [1K]
2. Rubidium
3. Antimony
4. Ytterbium
5. Einsteinium
8 0
2 years ago
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