Answer:
1.c
2.c
3.a
4.b
5.a
i think that's the answer
Answer:
pH = 4
Explanation:
Step 1: Given data
Concentration of H⁺ ions in the solution ([H⁺]): 10⁻⁴ M
Step 2: Calculate the pH of the solution
We will use the definition of pH.
pH = -log [H⁺]
pH = -log 10⁻⁴ M
pH = 4
The pH of the solution is 4. Considering the pH scale, given the pH is lower than 7, the solution is acidic.
Answer:
3
Explanation:
You need to remember that to measure the number of unparied electrons in an atom you need to undestard its electron configuration, and the electron configuration of phosphorus is 1s2 2s2 2p6 3s2 3p3, just the last state "3p3" have unpaired electron, and because a p state can fits 6 electrons, and here are only 3, that means that those 3 are unpaired.
Top to bottom:
osmosis
high
low
into
out of
sodium
Answer:
(a) pH = 1.0
(b) pH = 7.0
(c) 60 mL
Explanation:
(a) At the start of the titration there's no OH⁻ species yet.
pH = -log[H⁺]
And because HCl is a strong acid
[H⁺] = [HCl] = 0.1 M
Thus
pH = -log (0.1) = 1.0
(b) In every strong base-strong acid titration, the pH at the equivalence point is 7.0.
(c) Because<em> the concentration of HCl and NaOH are the same</em>, you would need<u> 30 mL of the NaOH solution to neutralize 30 mL of the HCl solution</u>, thus the total volume is 60 mL.
