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3 years ago

How do ethical concerns affect scientific research

Chemistry

1 answer:

Gwar [14]3 years ago

7 0

Answer:

Ethical concerns affect scientific research by adding boundaries to what can and cant be experimented on. An example is that its socially unacceptable to experiment on humans because its considered wrong and horrific, even at the expense of learning more about human nature and/or the human body.

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What mass of CuSO4 are needed to prepare 100 mL of a 0.10 M solution? grams

kaheart [24]

1.596 grams is the mass of CuSO4 needed to prepare 100 ml solution of 0.1 M solution.

Explanation:

Data given:

Volume of the solution = 100 ml or 0.1 litre

molarity of the solution = 0.10 M

mass of CuS $O_{4}$ = ?

atomic mass of CuS $O_{4}$ = 159.6 grams/mole

The mass will calculated by using the following relations:

number of moles = $\frac{mass}{atomic mass of 1 mole}$ equation 1

molarity = $\frac{number of moles}{volume}$ equation 2

putting the value of number of moles in equation 2

molarity = $\frac{mass}{atomic mass X Volume}$

mass = molarity x atomic mass x volume

mass = 0.1 x 0.1 x 159.6

= 1.596 grams

1.596 grams will form 100ml solution 0.1 M

5 0

3 years ago

Which element is in Group 2 and Period 7 of the Periodic Table?

miss Akunina [59]

Answer:

A) Radium

i don't think that group 2 has period 7, it has only up to period 6 so it's probably Radium :))

3 0

3 years ago

The molar mass of an unknown organic liquid (M ~ 100) is determined by placing 5 mL of the liquid in a weighed 125-mL conical fl

AlexFokin [52]

I think it should be A

6 0

4 years ago

A chemistry graduate student is given 125.mL of a 0.20M acetic acid HCH3CO2 solution. Acetic acid is a weak acid with =Ka×1.810−

Over [174]

Answer : The mass of sodium acetate is, 1.097 grams.

Explanation : Given,

The dissociation constant for acetic acid = $K_a=1.8\times 10^{-5}$

Concentration of acetic acid (weak acid)= 0.20 M

volume of solution = 125. mL

pH = 4.47

First we have to calculate the value of $pK_a$ .

The expression used for the calculation of $pK_a$ is,

$pK_a=-\log (K_a)$

Now put the value of $K_a$ in this expression, we get:

$pK_a=-\log (1.8\times 10^{-5})$

$pK_a=5-\log (1.8)$

$pK_a=4.74$

Now we have to calculate the concentration of sodium acetate (conjugate base or salt).

Using Henderson Hesselbach equation :

$pH=pK_a+\log \frac{[Salt]}{[Acid]}$

Now put all the given values in this expression, we get:

$4.47=4.74+\log (\frac{[Salt]}{0.20})$

$[Salt]=0.107M$

Now we have to calculate the mass of sodium acetate.

$\text{Concentration}=\frac{\text{Mass of }NaCH_3CO_2\times 1000}{\text{Molar mass of }NaCH_3CO_2\times \text{Volume of solution (in mL)}}$

$0.107M=\frac{\text{Mass of }NaCH_3CO_2\times 1000}{82g/mol\times 125mL}$

$\text{Mass of }NaCH_3CO_2=1.097g$

Therefore, the mass of sodium acetate is, 1.097 grams.

6 0

4 years ago

D. liquid

erastovalidia [21]

Answer: H2O

Explanation: The given balanced chemical reaction is,

This reaction is a reversible reaction.

The rate of forward reaction will be,

The rate of backward reaction will be,

And at equilibrium the rate of reaction is equal to the rate of backward reaction divided by the rate of forward reaction.

4 0

3 years ago