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Irina18 [472]
2 years ago
13

8. If you have 100 ml of 10X Buffer A, how could you prepare 450 ml of 1 X buffer A?

Chemistry
1 answer:
lakkis [162]2 years ago
6 0

We have that you can you prepare 450 ml of 1 X buffer A by adding 45ml of 10X buffer A with 405ml(450-45) of water

From the question we are told

If you have 100 ml of 10X Buffer A, how could you prepare 450 ml of 1 X buffer A

Generally the equation for the  Concentration  Volume relationship is mathematically given as

C1V1=C2V2\\\\Where\\\\C1=10X\\\\C2=1X buffer A\\\\V2=450ml \\\\Therefore\\\\V1=\frac{450*1}{10}\\\\V1=45ml

Therefore

You can you prepare 450 ml of 1 X buffer A by adding 45ml of 10X buffer A with 405ml(450-45) of water

For more information on this visit

brainly.com/question/17756498

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Using the following thermochemical data, what is the change in enthalpy for the following reaction? Ca(OH)2(aq) + HCl(aq) CaCl2(
sesenic [268]
Ca(OH)2(aq) + 2HCl(aq)------> CaCl2(aq) + 2H2O(l) ΔH-?

CaO(s) + 2HCl(aq)-----> CaCl2(aq) + H2O(l),  Δ<span>H = -186 kJ
</span>
CaO(s) + H2O(l) -----> Ca(OH)2(s), Δ<span>H = -65.1 kJ
</span>
1) Ca(OH)2 should be  reactant, so
CaO(s) + H2O(l) -----> Ca(OH)2(s) 
we are going to take as 
 Ca(OH)2(s)---->CaO(s) + H2O(l), and ΔH = 65.1 kJ

2) Add 2 following equations
Ca(OH)2(s)---->CaO(s) + H2O(l),                    and ΔH = 65.1 kJ
<span><u>CaO(s) + 2HCl(aq)-----> CaCl2(aq) + H2O(l), and ΔH = -186 kJ</u>

</span>Ca(OH)2(s)+CaO(s) + 2HCl(aq)--->CaO(s) + H2O(l)+CaCl2(aq) + H2O(l)

Ca(OH)2(s)+ 2HCl(aq)---> H2O(l)+CaCl2(aq) + H2O(l)
By addig these 2 equation, we got the equation that we are needed,
so to find enthalpy of the reaction, we need to add  enthalpies of reactions we added.
ΔH=65.1 - 186 ≈ -121 kJ
4 0
3 years ago
The diameter of a red blood cell is about 3 × 10−4 in. What is its diameter in centimeters?
lesantik [10]

Answer:

1 in. =2.54 cm

3*(10^-4)*2.54=7.62*10^-4

Explanation:

8 0
3 years ago
Read 2 more answers
Write a balanced equation for the complete oxidation reaction that occurs when methane (CH4) burns in air.
Lelechka [254]

Answer: The balanced equation for the complete oxidation reaction that occurs when methane (CH4) burns in air is CH_{4} + 2O_{2} \rightarrow CO_{2} + 2H_{2}O.

Explanation:

When a substance tends to gain oxygen atom in a chemical reaction and loses hydrogen atom then it is called oxidation reaction.

For example, chemical equation for oxidation of methane is as follows.

CH_{4} + O_{2} \rightarrow CO_{2} + H_{2}O

Number of atoms present on reactant side are as follows.

  • C = 1
  • H = 4
  • O = 2

Number of atoms present on product side are as follows.

  • C = 1
  • H = 2
  • O = 3

To balance this equation, multiply O_{2} by 2 on reactant side. Also, multiply H_{2}O by 2 on product side. Hence, the equation can be rewritten as follows.

CH_{4} + 2O_{2} \rightarrow CO_{2} + 2H_{2}O

Now, the number of atoms present on reactant side are as follows.

  • C = 1
  • H = 4
  • O = 4

Number of atoms present on product side are as follows.

  • C = 1
  • H = 4
  • O = 4

Since, the atoms present on both reactant and product side are equal. Therefore, this equation is now balanced.

Thus, we can conclude that balanced equation for the complete oxidation reaction that occurs when methane (CH4) burns in air is CH_{4} + 2O_{2} \rightarrow CO_{2} + 2H_{2}O.

4 0
3 years ago
How are journals helpful to scientists
Fofino [41]
They help keep track of notes and experaments
8 0
3 years ago
At 600. K how many moles of gas are in a 1.00 L cylinder at atmospheric pressure?
Anton [14]

Answer:

0.02moles

Explanation:

To answer this question, the general gas law equation is used. The General gas law is:

Pv = nRT

Where; P = standard atmospheric pressure (1 atm)

V = volume (L)

n = number of moles

R = Gas law constant

T = Temperature

For this question; volume = 1.00L, atmospheric pressure (P) = 1 atm, R = 0.0821 L-atm / mol K, T = 600K, n = ?

Therefore; Pv = nRT

n = PV/RT

n = 1 × 1/ 0.0821 × 600

n = 1/49.26

n = 0.0203moles

Hence, there are 0.02 moles of gas.

8 0
3 years ago
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