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2 years ago

Select the true statements about denaturation.

Chemistry

1 answer:

fiasKO [112]2 years ago

5 0

Answer:

The correct options are: Denaturation of an enzyme will cause a loss of its catalytic activity.

Egg white meringue contains denatured egg white proteins.

A denatured protein has a different tertiary structure than its native state.

Protein denaturation involves cleavage of its peptide bonds.

Explanation:

Protein denaturation is the breakdown of tertiary or quaternary junctions of proteins, which are the easiest to break compared to primary and secondary.

Denaturation can arise due to a change in pH or due to excess temperature. An enzyme is generally a protein and if it is subjected to acidic acids or high temperatures, it denatures, ceasing to perform its function.

Zymogen is a non-denatured INACTIVE proenzyme, that is why we consider that option false along with those that were not selected.

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I think the answer is C for this question

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What is the molarity of a naoh solution if 11.9 ml of a 0.220 m h2so4 solution is required to neutralize a 25.0-ml sample of the

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A 24.00 g sample contains 14.60 g Cl and 9.400 g B. What is the percent composition (by mass) of boron in this sample?

vaieri [72.5K]

Answer:

39.2 %

Explanation:

The following data were obtained from the question:

Mass of sample = 24 g

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Percentage composition of boron =?

The percentage composition (by mass) of boron in the sample can be obtained as illustrated below:

Percentage composition of boron = mass of B /mass of sample × 100

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2 years ago

BH+ClO4- is a salt formed from the base B (Kb = 1.00e-4) and perchloric acid. It dissociates into BH+, a weak acid, and ClO4-, w

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Answer:

The pH of 0.1 M BH⁺ClO₄⁻ solution is 5.44

Explanation:

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Also, water dissociation constant: $K_{w}$ = 1 × 10⁻¹⁴

The acid dissociation constant ( $K_{a}$ ) for the weak acid (BH⁺) can be calculated by the equation:

$K_{a}. K_{b} = K_{w}$

$\Rightarrow K_{a} = \frac{K_{w}}{K_{b}}$

$\Rightarrow K_{a} = \frac{1\times 10^{-14}}{1\times 10^{-4}} = 1\times 10^{-10}$

Now, the acid dissociation reaction for the weak acid (BH⁺) and the initial concentration and concentration at equilibrium is given as:

Reaction involved: BH⁺ + H₂O ⇌ B + H₃O+

Initial: 0.1 M x x

Change: -x +x +x

Equilibrium: 0.1 - x x x

The acid dissociation constant: $K_{a} = \frac{\left [B \right ] \left [H_{3}O^{+}\right ]}{\left [BH^{+} \right ]} = \frac{(x)(x)}{(0.1 - x)} = \frac{x^{2}}{0.1 - x}$