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3 years ago

How much sodium acetate is needed to make acetic acid neutral?

Chemistry

1 answer:

Zigmanuir [339]3 years ago

4 0

2.5 mL sodium acetate is needed to make 250 mL of the acetic acid.

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The reaction A + 2B ® products has been found to have the rate law, rate = k[A] [B]2. While holding the concentration of A const

Over [174]

Answer:

The rate of the reaction will increase by a factor of 9.

Explanation:

Hello,

In this case, considering the given second-order reaction, whose rate law results:

$r=k[A] [B]^2$

We easily infer that at constant concentration of A but tripling the concentration of B, we are going to obtain the following increasing factor while holding the remaining variables constant:

$Increase\ factor=\frac{r_{final}}{r_{initial}} =\frac{k[A][3*B]^2}{k[A][B]^2} =\frac{3^2}{1} \\Increase\ factor=9$

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3 years ago

All charges in a compound must have ?

MakcuM [25]

They must have both cations and anions.

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4 years ago

1.) 3.3482 hL =__________nL

Taya2010 [7]

Answer:

334820000000nL

Explanation:

Since 1hL=100000000000nL

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3 years ago

How many moles of NaCl can be formed from 6 moles of Cl2?

salantis [7]

Answer:

12 moles

Explanation:

7 0

3 years ago

A phosphate buffer is involved in the formation of urine. The developing urine contains H2PO4 and HPO42- in the same concentrati

Katen [24]

Answer:

The ionization equation is

$H_{2}PO_{4}^{-} +H_{2}O$ ⇄ $HPO_{4}^{-2} +H_{3}O^{+}$ (1)

Explanation:

The ionization equation is

$H_{2}PO_{4}^{-} +H_{2}O$ ⇄ $HPO_{4}^{-2} +H_{3}O^{+}$ (1)

As the Bronsted definition sais, an acid is a substance with the ability to give protons thus, H2PO4 is the acid and HPO42- is the conjugate base.

The Ka expression is the ratio between the concentration of products and reactants of the equilibrium reaction so,

$Ka = \frac{[HPO_{4}^{-2}] [H_{3}O^{+}]}{[H_{2}PO_{4}^{-}] [H_{2}O]} = 6.2x10^{-8}$

The pKa is

$-Log (Ka) = -Log (6.2x10^{-8}) = 7.2$

The pKa of H2CO3 is 6,35, thus this a stronger acid than H2PO4. The higher the pKa of an acid greater the capacity to donate protons.

In the body H2CO3 is a more optimal buffer for regulating pH due to the combination of the two acid-base equilibriums and the two pKa.

If the urine is acidified, according to Le Chatlier's Principle the equilibrium (1) moves to the left neutralizing the excess proton concentration.

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4 years ago