Answer: pH of the solution after the addition of 600.0 ml of LiOH is 7.
Explanation:
The given data is as follows.
Volume of = 900.0 ml = 0.9 L,
Molarity of = 0.18 M,
Hence, we will calculate the number of moles of as follows.
No. of moles = Molarity × Volume
= 0.18 M × 0.9 L
= 0.162 moles
Volume of NaOH = 600.0 ml = 0.6 L
Molarity of NaOH = 0.27 M
No. of moles of NaOH = Molarity × Volume
= 0.27 M × 0.6 L
= 0.162 moles
This shows that the number of moles of is equal to the number of moles of NaOH.
Also we know that,
As 1 mole of reacts with 1 mole of NaOH then all the hydrogen ions and hydroxide ions will be consumed.
This means that pH = 7.
Thus, we can conclude that pH of the solution after the addition of 600.0 ml of LiOH is 7.
Answer:
0.238 M
Explanation:
A 17.00 mL sample of the dilute solution was found to contain 0.220 M ClO₃⁻(aq). The concentration is an intensive property, so the concentration in the 52.00 mL is also 0.220 M ClO₃⁻(aq). We can find the initial concentration of ClO₃⁻ using the dilution rule.
C₁.V₁ = C₂.V₂
C₁ × 24.00 mL = 0.220 M × 52.00 mL
C₁ = 0.477 M
The concentration of Pb(ClO₃)₂ is:
Answer:
<h2>1.5 L</h2>Explanation:
The new volume can be found by using the formula for Boyle's law which is
Since we are finding the new volume
From the question we have
We have the final answer as
<h3>1.5 L</h3>Hope this helps you