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faltersainse [42]
3 years ago
8

You need a 35% alcohol solution. on hand, you have a 405 ml of a 30% alcohol mixture. you also have 80% alcohol mixture. how muc

h of the 80% mixture will you need to add to obtain the desired solution?
Chemistry
1 answer:
Bumek [7]3 years ago
4 0

You must add 45 mL of the 80 % alcohol to the 30 % alcohol to get a 35 % solution.

You can use a modified dilution formula to calculate the volume of 80 % alcohol

V1×C1 + V2×C2 = V3×C3

Let the volume of 80 % mixture 1 = <em>x</em> mL. Then the volume of the final 35 % mixture 3 = (405 + <em>x</em> ) mL

(<em>x</em> mL×80 % alc) + (405 mL×30 % alc) = (405 + <em>x</em>)mL × 35 % alc

80x + 12 150 = 14 175 + 35 x

45x = 2025

x = 2025/45 = 45

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Read 2 more answers
Calculate the pH of a buffer solution created by reacting 100 mL of 0.1 M NH3 with 90 mL of 0.1 M HNO3. (Remember, you can find
algol13

This question is asking for the pH of a buffer solution between ammonia and nitric acid, with given volumes and concentrations. At the end, the result turns out to be 10.488.

<h3>Buffers</h3>

In chemistry, buffers are known as substances attempting to hold a relatively constant pH by mixing and acid and a base (weak and strong). In such a way, for the substances given, the first step will be to calculate the consumed moles as they are mixed:

n_{NH_3}=0.1L*0.1mol/L=0.01mol\\\\n_{HNO_3}=0.09L*0.1mol/L=0.009mol

Now, since ammonia is in a greater proportion, one can calculate how much of it is left after being consumed by the nitric acid:

n_{NH_3}^{left}=0.01mol-0.009mol=0.001mol

And its new concentration:

[NH_3]=\frac{0.001mol}{0.1L+0.09L} =0.00526M

Next, with ammonia's ionization:

NH_3+H_2O\rightleftharpoons NH_4^++OH^-

We set up the equilibrium expression based on ammonia's Kb:

Kb=\frac{[NH_4^+][OH^-]}{[NH_3]}

Which can be solved by introducing x and using ammonia's Kb:

1.8x10^{-5}=\frac{x^2}{0.00526M}\\ \\

Then, we solve for x which is also equal to the concentration of ammonium and hydroxide ions in the solution:

x=\sqrt{0.00526*1.8x10^{-5}}=0.000308M

Ultimately, we calculate the pOH and then turn it into pH with:

pOH=-log(0.00308)=3.512\\\\pH=14-3.512=10.488

Learn more about buffers: brainly.com/question/24188850

6 0
2 years ago
The "Nutrition Facts" on a label of a 16 fluid ounce container of apple juice states that a serving size is 8 fluid ounces conta
spayn [35]

Answer:

a) 22 calories

b) 30 mg

Explanation:

Divide number of cal or mg of pot by 8 fl oz.

4 0
3 years ago
Coal can be used to generate hydrogen gas (a potential fuel) by thefollowing endothermic reaction.
Juliette [100K]

Answer:The statements b,c,d would lead to increased formation of more hydrogen gas and statements a, e and f would  lead to unchanged hydrogen concentration

Explanation:

Lechateliers principle can be used here to determine the effect  of changes observed in the system.

Lechateliers principle states that if  any reaction at equilibrium  is subjected to change in concentration, temperature and pressure or even in reaction conditions  then the equilibrium of the reaction would shift in such a way so that it can oppose the change .

So if any disturbance is caused to a reaction  at equilibrium hence  the equilibrium of reaction would shift in such a way so that it can counter balance the change caused to the reaction.

The above reaction is following:

C(s)+H₂O(g)→CO(g)+H₂(g)

The enthalpy change  of this reaction is positive and hence the reaction is endothermic in nature.

So the given changes would lead to the following  results:

a The addition of more amount of carbon C(s) would not lead to any further formation of hydrogen because carbon is added in solid state and Hydrogen gas is in gaseous state so the equilibrium for this given reaction would only change on addition of gaseous reactants as that would only lead to change in concentration.

b Since H₂O(g) is in gaseous state and a reactant and hence the addition of  H₂O(g) that is more reactant would lead to more formation of hydrogen gas according to lechatelier principle. The equilibrium would shift in such a way so that it can decrease the concentration of added H₂O(g) hence it would form H₂(g).

c Since the above reaction is endothermic in nature hence increasing the temperature of reaction would also shift the equilibrium of reaction towards more formation of H₂(g) that is in forward direction.

d When we increase the volume of reaction mixture that is we are increasing the amount of reactants hence the reaction would shift towards more formation of hydorgen gas.

e The catalyst does not change the position of equilibrium and hence no shift in position of equilibrium would be observed.So amount of hydrogen gas formed would remain unchanged.

f The addition of inert gas would not lead to any change to the reaction and equilibrium would be unaffected. Hence the formation of hydrogen gas would remain unchanged.

7 0
3 years ago
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