p [OH-] = -log[OH-]= -log ( 1x10^-11M) = 11
we know that
p[OH-] + p[H+] = 14
so p[H+] = 14- p[OH-] = 14- 11 = 3
pH = 3, answer
Answer:
The answers are in the explanation
Explanation:
For the equilibrium:
B(aq) + H₂O(l) ⇌ HB⁺(aq) + OH⁻(aq).
By LeChatelier's principle, the increase in the concentration of a reactant (for example) at equilibrium will change the system counteracting the increasing producing more product.
Thus,
A) Will the equilibrium constant for the reaction increase, decrease, or stay the same? Why?
.
The equilibrium constant is a thermodynamic constant that stay the same with the addition of a compound.
B) Will the concentration of HB⁺(aq) increase, decrease, or stay the same? Why?
By LeChatelier's principle, the addition of B will induce the formation of more HB⁺(aq) increasing the concentration.
C) Will the pH of the solution increase, decrease, or stay the same? Why?
As the addition of B induce the increasing of OH⁻, the pH of the solution will increase.
I hope it helps!
Answer: The empirical formula is 
Explanation:
If percentage are given then we are taking total mass is 100 grams.
So, the mass of each element is equal to the percentage given.
Mass of Ca= 55.6 g
Mass of S = 44.4 g
Step 1 : convert given masses into moles.
Moles of Ca =
Moles of S =
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For Ca = 
For S =
The ratio of Ca : S = 1:1
Hence the empirical formula is
To assume the empirical formula of a compound, you want the ratio of the moles of every element, and you discover that by means of the percent’s of the element as the element's mass.
As an instance, if a compound is 16% Carbon and 84% sulfur, you can round about that if you had a 100 gram sample of the compound, it would contain 16 grams of carbon & 84 grams of sulfur.
To look for the moles of carbon in that sample, you would distribute the mass by the atomic mass of carbon, so 16/12 = 1.3 moles. You do the similar calculation with the other elements. For Sulfur, you divide 84g by the atomic mass of sulfur, so 84/32 = 2.6moles of sulfur. You endure in this same way if there is more than 2 elements.
Lastly you find the ratio of the moles of every element. The unassuming way to do this is to look the element with the smallest number of moles and split the other moles by that number. In the above example 2.6 moles of Sulfur divided by 1.3 moles of Carbon equals 2. (Which is a 2:1 ratio) Therefore there is twice as numerous sulfurs as carbons in this compound, and the empirical formula is CS2.
The answer is C. The independent variable is the factor that is changed by the experimenter and impacts the dependent variable.
