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sesenic [268]
3 years ago
5

Sulfanomids warnings ​

Chemistry
1 answer:
cupoosta [38]3 years ago
4 0

Answer:

<em><u>Sulfanomides </u></em><em><u>Warnings </u></em>

<em><u>Sulfonamides may cause blood problems, especially if they're taken for a long period of time. These medicines can also cause a serious, even life-threatening, skin rash. Tell your doctor right away if you notice a rash or unusual skin changes.</u></em>

Explanation:

<h3 /><h3>Hope this helps you !!</h3>
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The answer I believe would be D) All of these
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3 years ago
a concentration solution of H2so4 is 59.4% by mass (m/m) and has a density of 1.83 g/mL. How many mL of the solution would be re
Blababa [14]

Answer: 41.5 mL

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

Molarity=\frac{n}{V_s}

where,

n = moles of solute

V_s = volume of solution in L

Given : 59.4 g of H_2SO_4 in 100 g of solution  

moles of H_2SO_4=\frac{\text {given mass}}{\text {molar mass}}=\frac{59.4g}{98g/mol}=0.61

Volume of solution =\frac{\text {mass of solution}}{\text {density of solution}}=\frac{100g}{1.83g/ml}=54.6ml

Now put all the given values in the formula of molality, we get

Molality=\frac{0.61\times 1000}{54.6ml}=11.2M

To calculate the volume of acid, we use the equation given by neutralisation reaction:

M_1V_1=M_2V_2

where,

M_1\text{ and }V_1 are the molarity and volume of stock acid which is H_2SO_4

M_2\text{ and }V_2 are the molarity and volume of dilute acid which is H_2SO_4

We are given:

M_1=11.2M\\V_1=mL\\M_2=0.30M\\V_2=1550mL

Putting values in above equation, we get:

11.2\times V_1=0.30\times 1550\\\\V_1=41.5mL

Thus 41.5 mL of the solution would be required to prepare 1550 mL of a .30M solution of the acid

4 0
3 years ago
Please I need this help me​
BaLLatris [955]

Answer:

first of all is that really chemistry

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1) x 2
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2In + 3Cd²⁺ ---> 2In³⁺ + 3Cd
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hope it helps ..............

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