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3 years ago

Which statement is correct concerning hereditary information?

Chemistry

1 answer:

Papessa [141]3 years ago

3 0

Answer:

the answer to this question is option A mark me as brainliest

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What is the molar mass of HBR

alexdok [17]

Answer:

Molar mass of bromine is equal to $80.9119$

Explanation:

The molar mass of HBr is equal to the sum of atomic weight of Bromine.

Atomic Weight of hydrogen is equal to $1.00794$

Atomic Weight of Bromine is equal to $79.904$

Molar mass of Bromine

= Atomic Weight of hydrogen + Atomic Weight of Bromine

Molar mass of Bromine $= 79.904 + 1.00794 = 80.9119$

3 0

3 years ago

Which of these is not a biomass source?

liberstina [14]

A biomass source is an natural material.

The sun is natural.

Manure is natural.

Wood Chips are natural.

Paper is natural and treated with unnatural substances.

7 0

3 years ago

Read 2 more answers

____________________ energy is the energy of movement.

neonofarm [45]

Thermal energy is the energy of movement.

7 0

3 years ago

How many atoms of hydrogen are in 0.500 mol of ch3oh molecules?

cestrela7 [59]

In 1 mol of CH3OH, you have 4 H-atoms (because 3 H-atoms are attached to the C-atom, and one H-atom in the OH group). That means in 0.500 mol of CH3OH, you have 2 H-atoms since it is halved. And then we have Avogadro's constant: 6.02 * 1023.

The question asks for how many hydrogen atoms there are in 0.500 mol CH3OH. Using the numbers that we have (Avogadro's constant and no. of H-atoms), the answer of the question will be something like:

<span>H-atoms in CH3OH = 2 * 6.02 * </span>1023<span> = ~1.2 * 10</span>24

8 0

3 years ago

What is the pH of a mixture of 0.042 M NaH2PO4 and 0.058 M Na2HPO4? Hint: The pKa of phosphate is 6.86.

AlekseyPX

Answer:

The pH value of the mixture will be 7.00

Explanation:

Mono and disodium hydrogen phosphate mixture act as a buffer to maintain pH value around 7. Henderson–Hasselbalch equation is used to determine the pH value of a buffer mixture, which is mathematically expressed as,

$pH=pK_{a} + log(\frac{[Base]}{[Acid]})$

According to the given conditions, the equation will become as follow

$pH=pK_{a} + log(\frac{[Na_{2}HPO_{4} ]}{[NaH_{2}PO_{4}]})$

The base and acid are assigned by observing the pKa values of both the compounds; smaller value means more acidic. NaH₂PO₄ has a pKa value of 6.86, while Na₂HPO₄ has a pKa value of 12.32 (not given, but it's a constant). Another more easy way is to the count the acidic hydrogen in the molecular formula; the compound with more acidic hydrogens will be assigned acidic and vice versa.

Placing all the given data we obtain,

$pH=6.86 + log(\frac{0.058}{0.042})$

$pH=7.00$

5 0

3 years ago