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Step2247 [10]
2 years ago
13

In order to complete his research project, Roger needs to make a mixture of 86 mL of a 36% acid solution from a 39% acid

Chemistry
2 answers:
nirvana33 [79]2 years ago
8 0

We have that the volume of the 39% acid solution that Roger needs to use to make the mixture.

x=74mL

From the question we are told that

Roger needs to make a mixture of 86 mL of a 36% acid solution from a 39% acid  solution and a 17% acid solution.

Hence

86 - x of the 17\% acid solution is taken by Rogers

Generally the equation for the mixture concentration is mathematically given as

C_m=\frac{39% solution concentration x volume of solution x 17% solution conc x volume of solution taken}{volume of solution mixture}

36 =\frac{ (39 * x + 17 * (86-x)) }{ 86}

x=74mL

For more information on this visit

brainly.com/question/17756498?referrer=searchResults

Zina [86]2 years ago
7 0

The volume of the 39% acid solution that Roger needs to use to make a mixture of 86 mL of a 36% acid solution is 74.27 mL.

The mixture of the acids solutions is given by:

CV = C_{1}V_{1} + C_{2}V_{2}    (1)      

Where:

C: is the concentration if the mixture = 36%  

V: is the total volume of the mixture = 86 mL

C₁: is the concentration of acid 1 = 39%

V₁: is the volume if acid 1 =?

C₂: is the concentration of acid 2 = 17%

V₂: is the volume of acid 2

The sum of V₁ and V₂ must be equal to V, so:

V = V_{1} + V_{2}

V_{2} = V - V_{1}  (2)

By entering equation (2) into (1), we have:

CV = C_{1}V_{1} + C_{2}(V - V_{1})

36\%*86 mL = 39\%*V_{1} + 17\%(86 mL - V_{1})

Changing the percent values to decimal ones:

0.36*86 mL = 0.39*V_{1} + 0.17(86 mL - V_{1})  

Now, by solving the above equation for V₁:

V_{1} = 74.27 mL  

Therefore, the volume of the 39% acid solution is 74.27 mL.

       

To learn more about mixture and solutions, go here: brainly.com/question/6358654?referrer=searchResults

I hope it helps you!  

         

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Answer:

Mass SrF2 produced = 38.63 g SrF2 produced

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[NO3^-]:  = 1.238 M

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[F^-] = 2.36*10^-5 M

Explanation:

Step 1: Data given

Volume of 2.888M strontium nitrate = 150.0 mL = 0.150 L

Volume of 3.076 M sodium fluoride = 200.0 mL = 0.200 L

Step 2 : The balanced equation

Sr(NO3)2(aq) + 2NaF(aq) → SrF2(s) + 2NaNO3(aq) → Sr2+ + 2F- + 2

Step 3: Calculate moles strontium nitrate

Moles Sr(NO3)2 = Molarity * volume  

Moles Sr(NO3)2 = 2.888 M * 0.150 L

Moles Sr(NO3)2 = 0.4332 moles

Step 4: Calculate moles NaF

Moles NaF = 3.076 M * 0.200 L

Moles NaF = 0.6152 moles

It takes 2 moles F^- to precipitate 1 mole Sr^2+, so F^- is limiting.

Step 5: Calculate limiting reactant

For 1 mol of Sr(NO3)2 we need 2 moles of NaF to produce 1 mol of SrF2 and 2 moles of NaNO3

NaF is the limiting reactant. It will completely be consumed (0.6152 moles).

Sr(NO3)2 is in excess. There will react 0.6152/2 = 0.3076 moles

Moles Sr^2+ precipitated by F^- = 0.3076

There will remain 0.4332 - 0.3076 = 0.1256 moles of Sr(NO3)2

Moles Sr^2+ no precipitated (left over) = 0.1256 moles

Step 6: Calculate moles SrF2  

For 1 mol of Sr(NO3)2 we need 2 moles of NaF to produce 1 mol of SrF2 and 2 moles of NaNO3

For 0.6152 moles NaF we have 0.6152/2 = 0.3076 moles of SrF2

Mass SrF2 produced:  0.3076 mol * 125.6 g/mol = 38.63 g SrF2 produced

Step 7: Calculate concentration of [Na+] and [NO3-]

Since both Na^+ and NO3^- are spectator ions, and the final volume is 150 ml + 200 ml = 350 ml (0.350 L), the concentrations of Na^+ and NO3^- can be calculated as follows:

[Na^+]:  (200 ml)(3.076 M) = (350 ml)(x M) and x = 1.758 M

[NO3^-]:  (150 ml)(2.888 M)(2) = (350 ml)(x M) = 1.238 M

Step 8: Calculate [Sr^2+] and [F^-]

[Sr^2+] = 0.1256 moles/0.350 L = 0.3589 M

To find [F^-], one needs the Ksp for SrF2.  There are several values listed in the literature. I am using a value of 2x10^-10.

SrF2(s) <==> Sr^2+(aq) + 2F^-(aq)

Ksp = [Sr^2+][F^-]²

2x10^-10 = (0.3589)(x)²

x² = 5.57*10^-10

x = [F^-] = 2.36*10^-5 M

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Now there are 6 atoms of carbon on the left side and 4 atoms on the right side. It can be balance by putting 3 in front of CO2 as shown below:

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