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3 years ago

How to titrate cocacola because of its dark colour

Chemistry

2 answers:

ivolga24 [154]3 years ago

7 0

Answer and Explanation

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All of the Information below is not owned by me, it is owned by CCBCMD.

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Colas are also carbonated beverages. The carbonation can produce some carbonic acid in the Cola, which would affect your results. Therefore, to ensure that you are only titrating the phosphoric acid you will use de-carbonated soda. This can easily be obtained by gently heating the soda, or as you may already know, by rapidly shaking the bottle. It is also important that we do not use diet Colas since the artificial sweeteners that they contain have acidic functional groups that will also interfere with the titration.

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Use a 25.00-mL pipet to deliver exactly 25.00 mL of room temperature, de-carbonated 

Cola into a 250-mL beaker. Check out a magnetic stir bar and gently add it to the 

beaker. Place the beaker on a stir plate. Set up a pH meter so that the probe is completely immersed, but in a way that the stir bar will not hit it. The tip of the probe 

has a thin glass membrane. Handle it with care! Position the beaker so that the stir bar 

is as close to the center of the beaker as possible for optimal stirring. It should stir 

rapidly enough to ensure thorough mixing but not so rapidly as to cause splattering. 

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Obtain about 75 mL of 0.0100 M NaOH in a beaker. Use this NaOH to fill a buret.

Remember that you should always rinse a buret 2-3 times with the solution that you are

about to put into it and remove air bubbles at the buret tip. If you do not remember how

The initial level of the NaOH should be at exactly

0.00 mL. Once the buret is ready, place it over the beaker containing the Cola

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Hope this helps! <3

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Bas_tet [7]3 years ago

4 0

Answer:

add baking soda maybe

Explanation:

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Calculate the concentrations of all species present in a 0.26 M solution of ethylammonium chloride (C2H5NH3Cl).

Alina [70]

Answer:

0.00000223

Explanation:

pKa for C2H5NH3+ = 10.7

pKw = 14.0

pKa + pKb = pKw

10.7 + pKb = 14.0

pKb = 14.0 - 10.7

pKb = 3.30

C2H5NH3Cl is a salt of ethylamine and HCl so it will dissolve in water to produce C2H5NH3^+ + Cl^-

The base hydrolysis reaction: C2H5NH3^+(aq) + H2O(l) <=> C2H5NH2(aq) + H3O^+(aq)

This reaction is described by Kb.

Kb = [C2H5NH2][H3O^+]/[C2H5NH3^+]

Let [C2H5NH2] = [H3O^+] = x,

so [C2H5NH3^+] = 0.26 - x

Kb = x^2/(0.26 - x) = 2.00 x 10^-11

Let's solve for x. In this equation, It is possible to solve without the use quadratic equation. So we can assume that 0.26 - x is approximately equal to 0.26. We won't know until we do the calculation.

We get: x^2 + 2.00 x 10^-11x - 4.99 x 10^-12 = 0

With the use of a quadratic calculator.

x = 2.23 x 10^-6 M = [C2H5NH2] = [H3O^+]

0.26 - x is just 0.26 M in this problem because 2.23 x 10^-6 M is insignificant.

[C2H5NH3^+] = 0.26 M = [Cl^-]

NOTE:

pH = -log [H3O^+] = -log(2.23 x 10^-6) = 5.65

Ka is the acid dissociation constant

Kb is the base dissociation constant

5 0

3 years ago

If 250 milliliters of Calcium Hydroxide is titrated with 345 milliliters of 0.75 molarity hydrobromic acid, what is the concentr

Bingel [31]

The balanced neutralization reaction here is:

Ca(OH)2 + 2HBr --> 2H2O + CaBr2

Notice that two moles of Her are required to neutralize every one mole of Ca(OH)2. This means that for however many moles of Her reacted, HALF as many moles of Ca(OH)2 reacted as well.

Moles of HBr reacted = 0.75 M x 0.345 L = 0.259 mol

Moles of Ca(OH)2 reacted = 0.259 mol / 2 = 0.130 mol

Concentration of Ca(OH)2 = 0.130 mol / 0.250 L = 0.52 M

4 0

3 years ago

I don’t get it plz help

d1i1m1o1n [39]

D=m/v. (Density equals mass over volume).
So in your case density = 4.2/6
Which equals 0.7
Your units will be grams over milliliters

So your answer is 0.7 g/ml

3 0

3 years ago

if the percent yield ofr the following reaction is 75% and 45.0g of NO2 are consumed with ercess water in the reaction. how many

NISA [10]

Answer:

30.8 grams of nitric acid are produced

Explanation:

Let's state the reaction:

3 NO₂ + H₂O → 2 HNO₃ + NO

If water is the excess reagent, then the limiting is the gas.

We convert the mass to moles:

45 g . 1 mol/ 46 g = 0.978 moles

Ratio is 3:2. 3 moles of gas can produce 2 moles of acid

Then, 0.978 moles may produce (0.978 . 2) /3 = 0.652 moles of acid

This is the 100% yield, but in this case, the percent yield is 75%

0.652 moles . 0.75 = 0.489 moles

Let's convert the moles to mass → 0.489 mol . 63g / 1mol = 30.8 g

6 0

3 years ago

Which physical property do plasmas and gases have in common?

sp2606 [1]

They both have charged particles
They have the same attractive forces between particles
They have the same space between particles
They create magnetic and electric fields

8 0

3 years ago

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