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Dominik [7]
3 years ago
5

In part 1 of lab 2 you will make and standardize a solution of naoh(aq). suppose in the lab you measure the solid naoh and disso

lve it into 100.0 ml of water. you then measure 0.2005 g of khp (kc8h5o4, 204.22 g/mol) and place it in a clean, dry 100-ml beaker, and then dissolve the khp in about 25 ml of water and add a couple of drops of phenolphthalein indicator. you titrate this with your naoh(aq) solution and find that the titration requires 9.82 ml of naoh(aq).
Chemistry
2 answers:
Nostrana [21]3 years ago
3 0
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Agata [3.3K]3 years ago
3 0

Answer:

0.100 M

Explanation:

KHP is used to standardize the NaOH solution, according to the following neutralization reaction.

KC₈H₅O₄ + NaOH → NaKC₈H₄O₄ + H₂O

We can establish the following relations.

  • The molar mass of KHP is 204.22 g/mol.
  • The molar ratio of KHP to NaOH is 1:1.

The moles of NaOH that reacted with 0.2005 g of KHP are:

0.2005gKHP.\frac{1molKHP}{204.22gKHP} .\frac{1molNaOH}{1molKHP} =9.818 \times 10^{-4} molNaOH

The molarity of NaOH is:

M=\frac{9.818 \times 10^{-4} mol}{9.82 \times 10^{-3}L} =0.100M

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Glycogen ________. Glycogen ________. forms the regulatory molecules known as enzymes serves as a structural component of human
jasenka [17]

Answer:

Glycogen in an important storage polysaccharide found in animal tissues.

Explanation:

Full question:

Glycogen ________

A) forms the regulatory molecules known as enzymes

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7 0
3 years ago
This for number 8 and 9
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If you measure the mass of a liquid is 11.50 g and its volume as 9.03 ml how many significant figures should its density value h
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To get a result with the best degree of precision, the number of significant figures should be equal to the smallest number of significant figures of the given numbers. In this case, the smallest is 3 as given by the number 9.03 mL.

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3 0
3 years ago
Read 2 more answers
How many grams of water can be produced from 4.6 grams of Hydrogen and 7.3 grams of Oxygen?
12345 [234]

Answer:

The answer to your question is 8.21 g of H₂O

Explanation:

Data

mas of water = ?

mass of hydrogen = 4.6 g

mass of oxygen = 7.3 g

Balanced chemical reaction

                   2H₂  +  O₂  ⇒   2H₂O

Process

1.- Calculate the atomic mass of the reactants

Hydrogen = 4 x 1 = 4 g

Oxygen = 16 x 2 = 32 g

2.- Calculate the limiting reactant

Theoretical yield = H₂/O₂ = 4 / 32 = 0.125

Experimental yield = H₂/ O₂ = 4.6/7.3 = 0.630

From the results, we conclude that the limiting reactant is Oxygen because the experimental yield was higher than the theoretical yield.

3.- Calculate the mass of water

                   32 g of O₂ ---------------- 36 g of water

                   7.3 g of O₂ ---------------   x

                          x = (7.3 x 36) / 32

                          x = 262.8 / 32

                          x = 8.21 g of H₂O

4 0
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