At equilibrium the concentrations of:
[HSO₄⁻] = 0.10 M;
[SO₄²⁻] = 0.037 M;
[H⁺] = 0.037 M;
There is initially very little H+ and no SO₄²⁻ in the solution. A salt is KHSO₄⁻. All KHSO₄⁻ will split apart into K⁺ and HSO₄⁻ ions. [HSO₄⁻] will initially be present at a concentration of 0.14 M.
HSO₄⁻ will not gain H⁺ to produce H₂SO₄ since H₂SO₄ is a strong acid. HSO₄⁻ may act as an acid and lose H⁺ to form SO₄²⁻. Let the final H⁺ concentration be x M. Construct a RICE table for the dissociation of HSO₄²⁻.
R
⇄ 
I 
C

E

×
for
. As a result,
![\frac{[H^+]. [SO_4^2^-]}{HSO_4^-} = K_a](https://tex.z-dn.net/?f=%5Cfrac%7B%5BH%5E%2B%5D.%20%5BSO_4%5E2%5E-%5D%7D%7BHSO_4%5E-%7D%20%3D%20K_a)
is large. It is no longer valid to approximate that
at equilibrium is the same as its initial value.

×
× 
Solving the quadratic equation for
since
represents a concentration;

Then, round the results to 2 significant figure;
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Answer:
24.525 g of sulfuric acid.
Explanation:
Hello,
Normality (units of eq/L) is defined as:

Since the sulfuric acid is the solute, and we already have the volume of the solution (500 mL) but we need it in liters (0.5 L, just divide into 1000), the equivalent grams of solute are given by:

Now, since the sulfuric acid is diprotic (2 hydrogen atoms in its formula) 1 mole of sulfuric acid has 2 equivalent grams of sulfuric acid, so the mole-mass relationship is developed to find its required mass as follows:

Best regards.
Answer:
1s2 2s2 2p6
Explanation:
ththe noble gas config. of neon
The answer is B.
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