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Anna [14]
2 years ago
13

How many milliliters of a 2.5% w/v chlorpromazine hydrochloride injection and how many milliliters of 0.9% w/v sodium chloride i

njection should be used to prepare 500 mL of a 0.3% w/v chlorpromazine hydrochloride injection
Chemistry
1 answer:
FrozenT [24]2 years ago
6 0

Answer:

Therefore, 107 ml of 2.5% w/v chlorpromazine hydrochloride injection and 393 ml of 0.9% w/v sodium chloride injection are needed to prepare 500 mL of a 0.3% w/v chlorpromazine hydrochloride injection

Explanation:

The method to be used in determining the proportions of each component to be used to get the desired mixture is known as alligation alternate.

Alligation alternate is a method by which to calculate the number of parts of two  or more components of a given strength when they are to be mixed to a desired  strength. The difference between the strength of the stronger component and the  desired strength indicates the number of parts of the weaker component to be used and the difference between the desired strength and the strength of the weaker  component indicates the number of parts of the stronger to be used.

Desired strength = 0.3%

Number of parts of 2.5% w/v chlorpromazine hydrochloride injection to be used = 0.9 - 0.3 = 0.6 parts

Number of parts of 0.9% w/v sodium chloride injection to be used = 2.5 - 0.3 = 2.2 parts

Total parts = 2.8 parts

2.8 parts of 0.3% w/v chlorpromazine hydrochloride injection = 500 ml

0.6 parts of 2.5% w/v chlorpromazine hydrochloride injection = 0.6 * 500 ml/2.8 = 107 ml of 2.5% w/v chlorpromazine hydrochloride injection

2.2 parts of 0.9% w/v sodium chloride injection = 2.2 * 500 / 2.8 = 393 ml of 0.9% w/v sodium chloride injection

Therefore, 107 ml of 2.5% w/v chlorpromazine hydrochloride injection and 393 ml of 0.9% w/v sodium chloride injection are needed to prepare 500 mL of a 0.3% w/v chlorpromazine hydrochloride injection

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Answer:

The answer to your question is below

Explanation:

Consider the reaction: P4 + 6Cl2 = 4PCl3.

a. How many grams of Cl2 are needed to react with 20.00 g of P4? ___68.7 g___________

                                P4      +      6Cl2      =      4PCl3

                          4(31) ---------- 12(35.5)

                         20     ----------    x

                    x = 20(12x35.5) / 4(31)

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b. You have 15.00 g. of P4 and 22.00 g. of Cl2, identify the limiting reactant and calculate the grams of PCl3 that can be produced as well as the grams of excess reactant remaining. LR____________ grams PCl3 _________ grams excess reactant ___________

                            P4      +      6Cl2      =      4PCl3

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                        15g               22g

I will use P4 to find the limiting reactant

                 

                     x = (15 x 426) / 124 = 51.5   The limiting reactant is Chlorine

                                                                  because we need 51.5 g and we only have 22g

Excess reactant

                 x = (22 x 124) / 426 = 6.4 g of P4

           Excess P4 = 15 g - 6.4 = 8.6 g of P4 in excess

Grams of PCl3 produced

                              426 g of Cl2 ----------------  550 g of PCl3

                                 22g of Cl2 ------------- -     x

            x = (22 x 550) / 426 = 28.4 g of PCl3

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Limiting reactant

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                                     28g           ---------------     x

x = (28 x 426) / 124

x = 96.2 g of Cl2 and we have 106.3 so Chlorine is the excess reactant and P4 is the limiting reactant.

Excess reactant = 106.3  - 96.2 = 10.1 g of Cl2 in excess

                   

                 

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