Answer is: H₂PO₄⁻ (d<span>ihydrogen phosphate).
Chemical reaction: HPO</span>₄²⁻(aq) + H⁺(aq) ⇄ H₂PO₄⁻(aq).
According to Bronsted-Lowry
theory acid are donor of protons and bases are acceptors of protons (the
hydrogen cation or H⁺). Hydrogen phosphate is Bronsted base and it can accept proton and become conjugate acid.
Easy stoichiometry conversion :)
So, for stoichiometry, we always start with our "given". In this case, it would be the 10.0 grams of NaHCO3. This unit always goes over 1.
So, our first step would look like this:
10.0
------
1
Next, we need to cancel out grams to get to moles. To do this, we will do grams of citric acid on the BOTTOM of the next step, so it cancels out. This unit in grams will be the mass of NaHCO3, which is 84.007. Then, we will do our unit of moles on top. Since this is unknown, it will be 1.
So, our 2nd step would look like this:
1 mole CO2
-----------------
84.007g NaHCO3
When we put it together: our complete stoichiometry problem would look like this:
10.0g NaHCO3 1mol CO2
---------------------- x -------------------------
1 84.007g NaHCO3
Now to find our answer, all we need to do is:
Multiply the two top numbers together (which is 10.0)
Multiply the two bottom numbers together (Which is 84.007)
And then....
Divide the top answer by the bottom answer.
10.0/84.007 is 0.119
So, from 10.0 grams of citric acid, we have 0.119 moles of CO2.
Hope I could help!
The Best Answer: 1 - (.47+.23) = 0.30
If Ne has a mole fraction of 0.47 (or 47/100) and Ar is 0.23, then H2(or He) has a mole fraction of 0.30
This means the gas mixture is 30/100 H2(or He).
7.85 x 0.30 = 2.355 atm
Answer:
0.367M
Explanation:
Molarity refers to the molar concentration of a solution. It can be calculated using the formula below:
Molarity = n/V
Where;
n = number of moles (mol)
V = volume (L)
According to the given information in this question;
n = 0.55 mole
V = 1.50 L
Molarity = 0.55/1.50
Molarity = 0.367M
