High 1 chemistry problem calculation about sodium sulfite deterioration .

1) The mass of sodium chloride can be found from the precipitation of silver nitrate (barium ions, sulfite ions, sulfate ions have been completely reacted, and there is only Na+, Cl-) in the solution), and the amount of NaCl is obtained from the formula n=m m, and the amount of Cl-is also known, and then the amount of BaCl2 is obtained by using N2, and the amount of its substance concentration c=n

2) After adding a sufficient amount of dilute sulfuric acid, the SO3 ion is oxidized to the SO4 ion, and the increased mass is the relative molecular mass of the sulfate ion - the relative molecular weight of the sulfite ion 96-80=16 So the amount of sulfite is n=

The amount of the substance of Na2SO3 is also m=n*m=

The quality score is:

The chemistry doesn't know how to send a short message.

Faint me to fight so much.

1) Na2SO3 + BACL2 = BaSO3 (precipitation) + NaClNa2SO4 + BACL2 = BaSO4 (precipitation) + NaClNaCl + AgNO3 = AGCL (precipitation) + nano32) Na2SO3 + H2SO4 = Na2SO4 + SO2 (gas) + H2O

Ah, isn't this question on our exam paper?

1). bacl2~~2nacl nacl~~~agcl↓x=

n（nacl）=m（nacl）/m（nacl）=n(bacl2)= n（nacl）/2=

c(bacl2)=n(bacl2)/v(bacl2)=2).baso3+h2so4=baso4+so2↑+h2o δm1mol 96-80=16

n(SO3 ions) =

n(na2so3)=

m(na2so3)=n(na2so3)*m(na2so3)=(na2so3)=

With the addition of BA (OH), there is a precipitate generated, in the addition of HCl, the precipitate is insoluble, it is completely deteriorated, there is partial dissolution, it is partially metamorphic, and the complete dissolution of the precipitate is not deterioration. I'm sorry, I know this.

1.Weigh a certain amount of sodium sulfite sample, add sulfuric acid acidified barium chloride, if there is precipitation, calculate, judge complete deterioration, partial deterioration, if there is no precipitation, no deterioration 2If the previous mass of sodium sulfite is known, it can be judged by calculation that it has completely deteriorated, partially deteriorated, or not deteriorated.

Sodium sulfite deteriorates, i.e., sodium sulfite solution is oxidized to produce sodium sulfate.

1. Proof of non-deterioration.

A small amount of solution was taken out, a sufficient amount of BACL2 was added to it, and after the precipitate was generated, dilute hydrochloric acid was added, and the precipitate was found to be completely dissolved.

This indicates that the sodium sulfite has not deteriorated.

2. Proof of partial deterioration.

The operation is the same as above, after the precipitation is generated, dilute hydrochloric acid is added, and it is found that most of the precipitate is dissolved, but there is still a small amount of precipitate that is not dissolved.

This indicates that some of the sodium sulfite is converted to Na2SO4.

If the amount of precipitate dissolved is relatively small, it doesn't matter.

Another sample solution was taken out, and a small amount of KMNO4 HCl solution was added dropwise, and the purple red color was found to be gone, indicating that there was still SO32- in the solution, and if it did not disappear, it would all deteriorate.

3. Proof of all deterioration.

The operation is the same as above, after adding dilute hydrochloric acid, the precipitate is completely insoluble, and it can be judged that all Na2SO3 has deteriorated.

If it is not possible to judge whether the precipitate is completely dissolved, add a little KMNO4 HCl solution according to the above method, if the purple red color does not disappear, it proves that SO32- is no longer present in the solution.

Good luck with your studies

The deterioration of sodium sulfite is oxidized to produce sodium sulfate, and the barium chloride solution can be added first, and then excessive hydrochloric acid can be added to observe the phenomenon.

The addition of barium chloride produces a white precipitate, and the addition of hydrochloric acid dissolves all of them, indicating that there is no deterioration.

The addition of barium chloride produces a white precipitate, and the partial dissolution of the precipitate after the addition of hydrochloric acid indicates partial deterioration.

The addition of barium chloride produces a white precipitate, and the precipitate does not dissolve after adding hydrochloric acid, indicating that all the precipitate has deteriorated.

1) Take a section of test Zheng Hu paper, take a small amount of solution with a glass rod, point it on the test paper, and compare it with the standard color card.

2）baso4s2o3

cl2h2o

10h+so4

6clso42-

ba2+baso4↓

3) Yes. Please shout bumper stop.

S = 32, Na = 23, no matter Na2SO3 or Na2SO4, there are Na2S, that is, there are 32 grams of S there is 2*23 = 46 grams of Na, if the mass fraction of sulfur is A, then the mass fraction of Na = 46A 32, and the mass fraction of oxygen = 1-A-46A 32

Step 1: Analyze the balance, sample and weighing paper.

Step 2: Beaker, glass rod.

Step 3: (1) The reason for the acidification of hydrochloric acid in the user of BaCl2 solution is (removal of sulfite ions); (2) The reason for adding too much BaCl2 solution is that after the sulfurous acid is deteriorated by ions, sulfate is generated, and excess barium chloride is added to allow the generated sulfate ions to react completely); (3) The way to test whether BaCl2 has been excessive is to take the supernatant dropwise and add dilute sulfuric acid to see if there is a white precipitate, and if there is a precipitate, it means that it is excessive, otherwise it is not excessive).

Step 4: Filter and wash the pellet. (1) The main instruments for filtration are (funnel, filter paper, glass rod, etc.); 2) The reason for the precipitation washing is (washing the soluble salts in the precipitation to ensure the accuracy of the experiment) (3) The method of washing the precipitation is (dilute with water, then filter, and repeat several times) (4) The method of judging whether the precipitation is washed is ( the solution after washing with water, add AgNO3 to see if there is a precipitation, if there is no precipitation, it means that it is washed, otherwise it is not washed, and there are CL ions.

Step 5: According to the amount of precipitate generated, the amount of sodium sulfate after spoilage is calculated, and then the amount of sodium sulfite spoiled (126 233)b, so its purity formula is: [a-126 233)b] a

Step 1: Scale, two pieces of paper of the same quality, medicine spoon; Step 2: Beaker, glass rod. Step 3:

1) exclude the interference of carbonate and sulfite on barium sulfate precipitation; (2) make the sulfate fully precipitated; (3) Take a little filtrate, drop in dilute sulfuric acid, if a white precipitate is generated, it proves that the added barium chloride has been excessive; Step 4: (1) funnel, filter paper, funnel holder, glass rod, beaker; (2) remove Na+ Ba+ H+ Cl- attached to the precipitate; 3) rinse the pellet with a small amount of distilled water 2 3 times; (4) Take a small amount of lotion and add silver nitrate solution to not generate precipitation, indicating that it has been washed; Step 5: [A-142 233)B] A 100%.

This is clear when you go through the experiment!