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3 years ago

How do you design a good scientific experiment?

Chemistry

1 answer:

kirill [66]3 years ago

7 0

Answer:

To design a good scientific research, there is a few things you need. You need to have an experiment first of course . You need an hypothesis, a conclusion, and research. Question,analysis, and observation.

Explanation:

If this helps : In fifth grade we did a scientific experiment that we had to present. I chose to do if bananas turned bad first under UV light or sun rays and my hypothesis was that they would turn bad under the sun-rays. My conclusion was that they didn't. My observation was written down in a notebook of what I saw with each passing day. Research was what I looked up about of course how long bananas lasted and how long they didn't.

Hope it helps :)

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A student creates a solution by dissolving some Na2SO4 (molar mass = 142.05 g/mol) in enough water to create 0.500 L of solution

NeX [460]

Answer : The mass of $Na_2SO_4$ is, 4.43 grams.

Explanation :

As we know that, when $Na_2SO_4$ dissolve in water then it dissociates to give 2 mole of sodium ion $Na^+$ and 1 mole of sulfate ion $SO_4^{2-}$

The chemical reaction will be:

$Na_2SO_4\rightarrow 2Na^++SO_4^{2-}$

Thus, the concentration of $Na_2SO_4$ = $\frac{\text{Concentration of }Na^+}{2}=\frac{0.125M}{2}=0.0625M$

First we have to calculate the moles of $Na_2SO_4$

$\text{Concentration of }Na_2SO_4=\frac{\text{Moles of }Na_2SO_4}{\text{Volume of solution}}$

$0.0625M=\frac{\text{Moles of }Na_2SO_4}{0.500L}$

$\text{Moles of }Na_2SO_4=0.0312mol$

Now we have to calculate the mass of $Na_2SO_4$

$\text{Mass of }Na_2SO_4=\text{Moles of }Na_2SO_4\times \text{Molar mass of }Na_2SO_4$

Molar mass of $Na_2SO_4$ = 142 g/mol

$\text{Mass of }Na_2SO_4=0.0312mol\times 142g/mol=4.43g$

Thus, the mass of $Na_2SO_4$ is, 4.43 grams.

6 0

3 years ago

Which of the following did Malthus fail to take into consideration?

saveliy_v [14]

Answer: humans would find more efficient ways of growing crops

Explanation:

4 0

3 years ago

Read 2 more answers

Gastric juice (pH 1.5) is produced by pumping HCl from blood plasma (pH 7.4) into the stomach. Calculate the amount of free ener

Annette [7]

Given question is incomplete. The complete question is as follows.

Gastric juice (pH 1.5) is produced by pumping HCl from blood plasma (pH 7.4) into the stomach. Calculate the amount of free energy required to concentrate the H in 1 liter of gastric juice at 37 degree of centigrade. Under cellular conditions, how many moles of ATP must be hydrolyzed to provide this amount of free energy? the free energy change for ATP hydrolysis under cellular conditions is about -58 kJ/mol. Ignore the effects of the transmembrane electrical potential.

Explanation:

The given data is as follows.

Gastric juice pH = 1.5, blood plasma pH = 7.4

Temperature = $37^{o}C$ = (37 + 273) K