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3 years ago

What does the atomic mass number of each atom represent.

Chemistry

1 answer:

mariarad [96]3 years ago

3 0

The atomic mass number tells us the number of neutrons and protons in the nucleus of an atom.

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This is due in five mintues please help

Fittoniya [83]

Answer:

Explanation:

Na, N, O, O, O

5 0

3 years ago

The titration of Na2CO3 with HCl has the following qualitative profile: a. Identify the major species in solution at points A-F.

exis [7]

Answer:

Answer is explained in the explanation section below.

Explanation:

Solution:

Note: This question is incomplete and lacks very important data to solve this question. But I have found the similar question which shows the profiles about which question discusses. Using the data from that question, I have solved the question.

a) We need to find the major species from A to F.

Major Species at A:

1. $Na_{2} CO_{3}$

Major Species at B:

1. $Na_{2} CO_{3}$

2. $NaHCO_{3}$

Major Species at C:

1. $NaHCO_{3}$

Major Species at D:

1. $NaHCO_{3}$

2. $H_{2}CO_{3}$

Major Species at E:

1. $H_{2}CO_{3}$

Major Species at F:

1. $H_{2}CO_{3}$

b) pH calculation:

At Halfway point B:

pH = pK $a_{1}$ + log[ $CO_{3}$ $.^{-2}$ ]/[H $CO_{3}$ $.^{-1}$ ]

pH = pK $a_{1}$ = 6.35

Similarly, at halfway point D.

At point D,

pH = pK $a_{2}$ + log [H $CO_{3}$ $.^{-1}$ ]/[H2 $CO_{3}$ ]

pH = pK $a_{2}$ = 10.33

8 0

3 years ago

How many atoms altogether make up one molecule of glucose

lilavasa [31]

Answer:

24 atoms makes altogether a molecule of glucose

7 0

4 years ago

A 48.3 mL sample of gas in a cylinder is warmed from 22 C, 87 C to 0.0 C what is the final temperature

snow_lady [41]

The answer is:

the volume stays the same. it is the pressure that increases

7 0

3 years ago

A solution made by dissolving 33 mg of insulin in 6.5 mL of water has an osmotic pressure of 15.5 mmHg at 25°C. Calculate the mo

Liula [17]

<u>Answer:</u> The molar mass of the insulin is 6087.2 g/mol

<u>Explanation:</u>

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

$\pi=iMRT$

Or,

$\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT$

where,

$\pi$ = osmotic pressure of the solution = 15.5 mmHg

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of solute (insulin) = 33 mg = 0.033 g (Conversion factor: 1 g = 1000 mg)

Volume of solution = 6.5 mL

R = Gas constant = $62.364\text{ L.mmHg }mol^{-1}K^{-1}$

T = temperature of the solution = $25^oC=[273+25]=298K$

Putting values in above equation, we get:

$15.5mmHg=1\times \frac{0.033\times 1000}{\text{Molar mass of insulin}\times 6.5}\times 62.364\text{ L.mmHg }mol^{-1}K^{-1}\times 298K\\\\\text{molar mass of insulin}=\frac{1\times 0.033\times 1000\times 62.364\times 298}{15.5\times 6.5}=6087.2g/mol$

Hence, the molar mass of the insulin is 6087.2 g/mol

8 0

3 years ago