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2 years ago

If concentrated sulfuric acid is spilled during the experiment, what is the proper procedure for cleaning the spill?

1 answer:

5 0

Sulfuric acid (H2SO4) is a strong acid which should be neutralized with a base. Ideally, sodium bicarbonate (NaHCO3) is used to treat acid spills. The reaction is as follows:

H2SO4 + 2NaHCO3 → Na2SO4 + 2H2O + 2CO2

Bubbles will be formed as CO2 is released. Once all H2SO4 has been neutralized the bubbles will stop. The pH of the spill after neutralization can be checked with a pH and should be between 6-9. If optimal pH is observed the waste can be disposed into a proper container and the work station can be cleaned with a paper towel.

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identify the reagents necessary to achieve each of the following transformations o3 dms, pcc, ch2cl, h2so4,h2o,hgso4

hoa [83]

the reagents necessary to convert alcohol to ketone $Na_2Cr_2O_7 , H_2O$ which involves oxidation of alcohols.

<h3>What is oxidation of alcohols?</h3>

Alcohol oxidation is a significant organic chemistry process. Secondary alcohols can be oxidized to produce ketones, while primary alcohols can be oxidized to produce aldehydes and carboxylic acids.
In contrast, tertiary alcohols cannot be oxidized without the C-C bonds in the molecule being broken.
In order to cause primary alcohols to oxidize into aldehydes

$Cr_2O_7 ^-^2$ (dichromate)
$CrO_3$ /pyridine (Collins reagent)
Chromium pyridinium compound (PCC)
Dichromate of pyridinium (PDC, Cornforth reagent)
Periodinane by Dess-Martin
Oxalyl chloride with dimethylsulfoxide (DMSO) for Swern

oxidation of secondary alcohols to ketones

$Cr_2O_7 ^-^2$ (dichromate)
$CrO_3$ /pyridine (Collins reagent)
Chromium pyridinium compound (PCC)
Dichromate of pyridinium (PDC, Cornforth reagent)
Periodinane by Dess-Martin
Oxalyl chloride and dimethyl sulfoxide (DMSO) (Swern oxidation)
$CrO_3, H_2SO_4$ /acetone (Jones oxidation)
Acetone with aluminum isopropoxide (Oppenauer oxidation)

To learn more about oxidation of alcohols with the given link

brainly.com/question/7207863

#SPJ4

Question:

Identify the reagents necessary to achieve each of the following transformations

$a. O_3 , DMS$

$b.H_2SO_4 , H_2O , HgSO_4$

$c.Na_2Cr_2O_7 , H_2O$

$d.Fe ^ {2+}, NaOH$

3 0

2 years ago

Which of the following are considered pure substances?

Tanzania [10]

Element. Everything is else is a mixture, therefore not pure.

8 0

3 years ago

Read 2 more answers

In E. coli, the enzyme hexokinase catalyzes the reaction: Glucose + ATP → glucose 6-phosphate + ADP The equilibrium constant, Ke

kondor19780726 [428]

Answer:

Explanation:

Glucose + ATP → glucose 6-phosphate + ADP The equilibrium constant, Keq, is 7.8 x 102.

In the living E. coli cells,

[ATP] = 7.9 mM;

[ADP] = 1.04 mM,

[glucose] = 2 mM,

[glucose 6-phosphate] = 1 mM.

Determine if the reaction is at equilibrium. If the reaction is not at equilibrium, determine which side the reaction favors in living E. coli cells.

The reaction is given as

Glucose + ATP → glucose 6-phosphate + ADP

Now reaction quotient for given equation above is

$q=\frac{[\text {glucose 6-phosphate}][ADP]}{[Glucose][ATP]}$

$q=\frac{(1mm)\times (1.04 mm)}{(7.9mm)\times (2mm)} \\\\=6.582\times 10^{-2}$

so,

$q$ ⇒ following this criteria the reaction will go towards the right direction ( that is forward reaction is favorable until q = Keq

4 0

3 years ago

Assuming the volumes are additive, what is the [Cl−] in a solution obtained by mixing 297 mL of 0.675 M KCl and 664 mL of 0.338

Elden [556K]

Answer: The concentration of chloride ions in the solution obtained is 0.674 M

Explanation:

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}$ .....(1)

For KCl:

Molarity of KCl solution = 0.675 M

Volume of solution = 297 mL

Putting values in equation 1, we get:

$0.675=\frac{\text{Moles of KCl}\times 1000}{297}\\\\\text{Moles of KCl}=\frac{(0.675mol/L\times 297)}{1000}=0.200mol$

1 mole of KCl produces 1 mole of chloride ions and 1 mole of potassium ion

Moles of chloride ions in KCl = 0.200 moles

For magnesium chloride:

Molarity of magnesium chloride solution = 0.338 M

Volume of solution = 664 mL

Putting values in equation 1, we get:

$0.338=\frac{\text{Moles of }MgCl_2\times 1000}{664}\\\\\text{Moles of }MgCl_2=\frac{(0.338mol/L\times 664)}{1000}=0.224mol$

1 mole of magnesium chloride produces 2 moles of chloride ions and 1 mole of magnesium ion

Moles of chloride ions in magnesium chloride = $(2\times 0.224)=0.448mol$

Calculating the chloride ion concentration, we use equation 1:

Total moles of chloride ions in the solution = (0.200 + 0.448) moles = 0.648 moles

Total volume of the solution = (297 + 664) mL = 961 mL

Putting values in equation 1, we get:

$\text{Concentration of chloride ions}=\frac{0.648mol\times 1000}{961}\\\\\text{Concentration of chloride ions}=0.674M$

Hence, the concentration of chloride ions in the solution obtained is 0.674 M

5 0

3 years ago

Help ASAP pleaseeee thank you

Artyom0805 [142]

The correct answer is B. balance

8 0

2 years ago