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galina1969 [7]
3 years ago
10

A 30.0 mL sample of 2.3 M Cu(OH)2 sample was titrated to with 48.5 mL of HNO3 to find

Chemistry
1 answer:
navik [9.2K]3 years ago
8 0

Answer:

2.8 M HNO3

Explanation:

                 Cu(OH)2 + 2HNO3 ---> Cu(NO3)2 + 2H2O

                 1 mol           2 mol

The number of moles Cu(OH)2 in the sample:

2.3 mol/L*0.0300L = 0.069 mol

The number of moles HNO3  in the solution of HNO3 that was used for titration

x mol/L*0.0485L = 0.0485x mol

From equation we can see that number of moles HNO3 = 2 times number of moles Cu(OH)2.

So, we can write

0.0485x = 2*0.069

x = 2*0.069/0.0485 = 2.8 M HNO3

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Question 34 (1 point)
Grace [21]

Answer:

8.33 atm

Explanation:

Xe is   5  out of (4+5)   or   5 / 9 ths of the gas present

  5/9  * 15 atm = 8.33 atm

4 0
1 year ago
If 16.9 kg of Al2O3(s), 57.4 kg of NaOH(l), and 57.4 kg of HF(g) react completely, how many kilograms of cryolite will be produc
hodyreva [135]

Answer: 69.72 kg of cryolite will be produced.

Explanation:

The balanced chemical equation is:

Al_2O_3(s)+6NaOH(l)+12HF(g)\rightarrow 2Na_3AlF_6+9H_2O

To calculate the moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}

moles of Al_2O_3 = \frac{16.9\times 1000g}{102g/mol}=165.7moles

moles of NaOH = \frac{57.4\times 1000g}{40g/mol}=1435moles

moles of HF = \frac{57.4\times 1000g}{20g/mol}=2870moles

As 1 mole of Al_2O_3 reacts with 6 moles of NaOH

166 moles of  Al_2O_3 reacts with = \frac{6}{1}\times 166=996 moles of NaOH

As 1 mole of Al_2O_3 reacts with 12 moles of HF

166 moles of  Al_2O_3 reacts with = \frac{12}{1}\times 166=1992 moles of HF

Thus Al_2O_3 is the limiting reagent.

As 1 mole of Al_2O_3 produces = 2 moles of cryolite

166 moles of  Al_2O_3 reacts with = \frac{2}{1}\times 166=332 moles of cryolite

Mass of cryolite (Na_3AlF_6) = moles\times {\text {molar mass}}=332mol\times 210g/mol=69720g=69.72kg

Thus 69.72 kg of cryolite will be produced.

8 0
3 years ago
A chemist determined by measurements that 0.050 moles of aluminum participated in a chemical reaction. Calculate the mass of alu
Law Incorporation [45]

Answer:

13.5 g

Explanation:

This question is solved easily if we remember that the number of moles is obtained by dividing the mass into the atomic weight or molar mass depending if we are referring to elements or molecules.

Therefore, the mass of aluminum in the reaction will the 0.050 mol Al times the atomic weight of aluminum.

number of moles = n = mass of Al / Atomic Weight Al

⇒ mass Al = n x Atomic Weight Al = 0.050 mol x 27 g mol⁻¹

                                                         = 13.5 g

We have three significant figures in 0.050 and therefore we should have three significant figures in our answer.

           

8 0
3 years ago
Drag and drop each phrase below the type of weathering it describes.
iren2701 [21]

Answer:

Mechanical weathering

A. does not change rock composition

C. abrasion

F. ice wedging

Chemical weathering

B. oxidabon

D. changes rock composition

E. acid rain

Explanation:

5 0
2 years ago
Read 2 more answers
In which of these statements are protons, electrons, and neutrons correctly compared?
algol13
The statement that correctly compares protons, electrons, and neutrons is, "Quarks are present in protons and neutrons but not in electrons". Quarks are tiny particles which compose the neutrons and protons. These quarks in protons and neutrons are linked together by gluons. 
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3 years ago
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