Answer:
0.4515 M
Explanation:
In case of titration , the following formula can be used -
M₁V₁ = M₂V₂
where ,
M₁ = concentration of acid ,
V₁ = volume of acid ,
M₂ = concentration of base,
V₂ = volume of base .
from , the question ,
M₁ = ? M
V₁ = 10.0 mL
M₂ = 0.100 M
V₂ = 45.15 mL
Using the above formula , the molarity of acid , can be calculated as ,
M₁V₁ = M₂V₂
M₁ * 10.0mL = 0.100 M * 45.15 mL
M₁ = 0.4515 M
Hence, the concentration of the acetic acid = 0.4515 M
The answer to this question is C) ALO2
Explanation:
Reliability can be improved by completing each temperature more than once and calculating an average.
Answer:
2H+ (aq) + 2OH-(aq)→ 2H2O (l)
Explanation:
Step 1: the balanced equation
2HBr(aq) + Ba(OH)2(aq) ⟶ 2H2O(l)+BaBr2(aq)
Step 2: The net ionic equation
The net ionic equation, for which spectator ions are omitted - remember that spectator ions are those ions located on both sides of the equation - will , after canceling those spectator ions in both side (Ba^2+ and Br-), look like this:
2H+ (aq) + 2OH-(aq)→ 2H2O (l)
To determine the mass of xenon tetrafluoride, we need to know first the number of fluorine atoms present in <span>oxygen difluoride. We need to convert first the mass into moles then make use of the relation of the elements from the chemical formula. Then, use the avogadro's number to convert it to number of atoms. Then, we do the reverse of the steps above but this time for </span><span>xenon tetrafluoride.
25.0 g OF2 ( 1 mol / 54 g ) ( 2 mol F / 1 mol OF2 ) ( 6.022 x10^23 atoms F / 1 mol F ) ( 1 mol / 6.022x10^23 atoms) ( 1 mol XeF4 / 4 mol F ) (207.3 g / 1 mol XeF4) = 47.99 g XeF4</span>
