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3 years ago

Which of the following instruments is used during a titration? test tube beaker burette crucible

1 answer:

4 0

I believe the correct answer would be the third option. It is the burette that is the apparatus that is used in titration. It is the best apparatus to use since you can easily control the amount you add to the sample solution. Also, you can easily read off the volume that was added.

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The absorbance of a chlorophyll a standard solution in ethanol (density = 0.785 g/mL) is measured in

Dmitry_Shevchenko [17]

Let A= ebc 
 0.765 = 86,300*1.3*c 

Solve for c = approximately 7E-6 Molar
= mols/L soln. 
g = 7E-6*893.49
= about 0.006 g chlorophyll/L soln. 

1000 x 0.785 = 785 g ethanol. 
Conc. = about 0.006g chlorophyll/785 g soln. 

Change that to ppm. by using formula:
(0.006/785)*1E6

5 0

2 years ago

Read 2 more answers

Consider the following first-order reaction: A → B. The concentration of A at the start of the reaction is 4.17 M and after 4.84

valina [46]

Answer : The value of rate constant is, $0.0327s^{-1}$

Explanation :

First we have to calculate the rate constant, we use the formula :

Expression for rate law for first order kinetics is given by:

$k=\frac{2.303}{t}\log\frac{a}{a-x}$

where,

k = rate constant = ?

t = time passed by the sample = 4.84 s

a = initial concentration = 4.17 M

a - x = concentration after time 4.84 s = 3.56 M

Now put all the given values in above equation, we get

$k=\frac{2.303}{4.84}\log\frac{4.17}{3.56}$

$k=0.0327s^{-1}$

Therefore, the value of rate constant is, $0.0327s^{-1}$

4 0

2 years ago

Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it

Sauron [17]

Answer:

The concentration of COF₂ at equilibrium is 0.296 M.

Explanation:

To solve this equilibrium problem we use an ICE Table. In this table, we recognize 3 stages: Initial(I), Change(C) and Equilibrium(E). In each row we record the concentrations or changes in concentration in that stage. For this reaction:

2 COF₂(g) ⇌ CO₂(g) + CF₄(g)

I 2.00 0 0

C -2x +x +x

E 2.00 - 2x x x

Then, we replace these equilibrium concentrations in the Kc expression, and solve for "x".

$Kc=8.30=\frac{[CO_{2}] \times [CF_{4}] }{[COF_{2}]^{2} } =\frac{x^{2} }{(2.00-2x)^{2} } \\8.30=(\frac{x}{2.00-2x} )^{2} \\\sqrt{8.30} =\frac{x}{2.00-2x}\\5.76-5.76x=x\\x=0.852$

The concentration of COF₂ at equilibrium is 2.00 -2x = 2.00 - 2 × 0.852 = 0.296 M

6 0

2 years ago

What is the total number of protons, neutrons, and electrons in a cadmium, Cd, atom that has a mass number of 112?

Triss [41]

Answer:

Number of Protons 48

Number of Neutrons 64

Number of Electrons 48

Explanation:

The mass number of an atom is the sum of the number of protons and neutrons in the nucleus of that atom

6 0

2 years ago

Ni4+ + _____e- LaTeX: \longrightarrow⟶ Nix+

stich3 [128]

Kdd was he e shxiuw r thai ed

4 0

2 years ago