Which step of the scientific method involves obtaining resources for your question

Chemistry

1 answer:

bezimeni [28]3 years ago

5 0

Answer:

c-do background research.

Explanation:

The scientific methods exposes the way scientists carry out their investigation and how findings are reported and at times discarded. It is systematic way of studying perceived observations in the environment.

During the course of an investigation, scientists may seek to find out about the prevailing knowledge about a phenomena and the level of research that might have been done in that regard. It is proper for such a scientist to do a background research by searching for related journals and publications in that field.

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A solution containing a mixture of lactic acid and lactate was found to have a pH of 4.26. Calculate the ratio of the lactate co

Aleks04 [339]

Given :

pH of solution of mixture of lactic acid and lactate is 4.26 .

To Find : $log( \dfrac{[ \text{Conc. of lactate}]}{[\text{Conc . of lactic acid }]}) = 0.4$

The ratio of the lactate concentration to the lactate .

Solution :

We know , pKa of lactic acid is :

pKa = 3.86 .

Now , the solution of lactic acid and lactate is a buffer solution .

So , pHof buffer acid is given by :

$pH=pKa+log(\dfrac{[Salt]}{[Acid]})$

Putting all given values :

$log( \dfrac{[ \text{Conc. of lactate}]}{[\text{Conc . of lactic acid }]}) = 0.4$

Taking anti log both the sides , we get :

$\dfrac{[ \text{Conc. of lactate}]}{[\text{Conc . of lactic acid }]} = 2.51$

Therefore , the ratio of the lactate concentration to the lactate is 2.51 .

Hence , this is the required solution .

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Calculate the molar concentration of HA (90.2 g/mol) in a solution that has a specific gravity of 1.24 and is 64% HNO3 (w/w).

ser-zykov [4K]

Answer:

Explanation:

Hello,

In this case, considering the given specific gravity we are to compute the density of the 64% HNO3 solution:

$\rho=1.24*1g/mL=1.24g/mL$

In such a way, since the given solution of nitric acid is 64 % by mass, we've got:

$\frac{64gHNO_3}{100g\ solution}$

Thus, by using the previously computed density and the molar mass of HA (90.2 g/mol) we can compute the required molar concentration as follows:

$M=\frac{(100g-64g)HA}{100g\ solution}*\frac{1.24g\ solution }{1mL \ solution}*\frac{1000mL\ solution}{1L\ solution}*\frac{1molHA}{90.2gHA} \\\\M=4.95M$