The answer is in the picture which is given below:
Answer: It is a basic solution with pH =8.51
Explanation:
We were given that hydroxide ion concentration [OH-] as 3.26 x 10-6 M
But We know thar
[OH-] [H+] = 1 × 10^-14
To get the Hydrogen ion [H+] concentration, we have that
[H+] = 1 × 10^-14 M/[OH-]
= 1 × 10^-14 M/3.26 x 10-6 M
= 3.067 x 10^-9 M
But, pH = - log [H+]
Therefore,
pH = - log (3.067 x 10^-9)
pH=8.51
when pH > 7, The solution is basic, therefore a solution with pH =8.51 is basic.
The chemical with the lowest point is helium
Answer:
We have to add 17.2 grams of aluminium bromide
Explanation:
Step 1: Data given
Molarity of the aluminum bromide solution = 0.215 M
Volume = 300 mL = 0.300 L
Molar mass aluminium bromide = 266.69 g/mol
Step 2: Calculate moles Aluminium bromide
moles AlBr3 = volume * molarity
Moles AlBr3 = 0.300 L * 0.215 M
Moles AlBR3 = 0.0645 moles
Step 3: Calculate mass aluminium bromide
Mass aluminium bromide = moles AlBr3 * molar mass AlBr3
Mass aluminium bromide = 0.0645 moles * 266.69 g/mol
Mass aluminium bromide = 17.2 grams
We have to add 17.2 grams of aluminium bromide
A or C for number 4 and for number 5 it could be C
