answer

watching

views

6 Nov 2019

A whitesolid was known to be the anhydrous form of either sodium carbonateor sodium bicarbonate (sodium hydrogen carbonate). Both react withhydrochloric acid to give sodium chloride, water, and carbondioxide, but the mole proportions are not the same

Write themolecular equation for the reaction of sodium carbonate withhydrochloric acid. Do not include physical states in youranswer.

Write themolecular equation for the reaction of sodium bicarbonate withhydrochloric acid. Do not include physical states in youranswer.

It wasfound that 0.4534 g of the solid reacted with 30.08 mL of0.2844 M HCl, and that theaddition of more acid caused the formation of no more carbondioxide. Identify the unknown solid. Enter "carbonate" for sodiumcarbonate or "bicarbonate" for sodium bicarbonate.

answer

watching

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Keith LeannonLv2

6 Mar 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

Baking soda is pure sodium bicarbonate, NaHCO3, which dissolves and dissociates in water into thesodium ion and the bicarbonate ion. As most students know from demonstrations in grade school or athome, it can be mixed with vinegar for a rapid and entertaining chemical reaction that generates carbondioxide gas bubbling out of the reaction mixture.

The overall reaction can be written as:CH3COOH (aq) + Na+(aq) + HCO3â(aq) â Na+(aq) + CH3COOâ(aq) + H2O(l) + CO2(g) in which the sodium ion is a spectator ion.

Baking soda or baking powder can be used in recipes as a leavening agentâthat is, to produce carbondioxide gas to make dough or batter rise. Recipes using baking soda must include a separate acidicingredient such as buttermilk or vinegar. Recipes that do not include the separate addition of an acidicingredient usually require baking powder instead. Baking powder has a solid organic acid mixed in withthe baking soda, so that when the mixture is dissolved, the acid and sodium bicarbonate react with eachother. While commercial baking powder involves slightly more complicated chemistry, a good substitutefor baking powder can be made by adding baking soda to an acid such as potassium hydrogen tartrate(potassium bitartrate or cream of tartar). The formula for potassium hydrogen tartrate is KH C4H4O 6 . Your task is to devise a suitable substitute for baking powder by calculating the mass of cream of tartar in grams required to react with 10.00 g of baking soda. There should be enough cream of tartar added so that all of the baking soda will react to make carbon dioxide gas, but no more cream of tartar than that.

The lab is for CHEM II and it is taken out of a lab paq. Beloware the materials used.

Classify your ions according to the following three groups.

Several of the cations belong to more

than one group.

Group 1: Anions that WILL NOT PRECIPITATE in the presence of

silver nitrate.

Group 2: Anions that WILL PRECIPITATE in the presence ofsilver

nitrate and the resulting

precipitates WILL DISSOLVE upon acidification with nitric

acid.

Group 3: Anions that WILL PRECIPITATE in the presence ofsilver

nitrate and the resulting

precipitates WILL NOT DISSOLVE upon acidification withnitric

acid.

A. Write a net ionic equation for any reaction that producesa

precipitate.

B. Identify the anions that produce gas upon addition of

HCl.

C. Identify the anions that do not precipitate with silver

nitrate.

D. Identify the anions that react with silver nitrate toform

precipitates that dissolve when

acidified with nitric acid.

E. Identify the anions that react with silver nitrate toform

precipitates that do not dissolve when

acidified with nitric acid.

F. What simple test (other than a specific confirmationtest)

would distinguish between CO3 2-

and NO3 - ?

Here are the materials we used

1 Ammonium Molybdate, 0.2 M - 2 mL in Pipet

1 Aqueous Ammonia, 6 M, NH4OH - 4 mL in Pipet

1 Barium Chloride, 0.3 M - 2 mL in Pipet

1 Hydrochloric Acid, 6 M - 8 mL in Dropper Bottle

1 Nitric Acid, 6 M - 2.5 mL in Pipet

1 Organic Reagent - 1.5 mL in Vial

2 Pipet, Empty Short Stem

1 Silver Nitrate, 0.1 N - 6 mL in White Dropper

Bottle

1 Sodium Bromide, 0.1 M - 2.5 mL in Pipet

1 Sodium Carbonate, 0.25 M - 2.5 mL in Pipet

1 Sodium Chloride, 0.1 M - 2.5 mL in Pipet

1 Sodium Iodide, 0.1 M - 2.5 mL in Pipet

1 Sodium Phosphate, 0.1 M - 2.5 mL in Pipet

1 Sodium Sulfate, 0.1 M - 2.5 mL in Pipet

1 Sodium Sulfide, 0.1 M - 2.5 mL in Pipet

1 Unknown - 5 mL in Pipet

burgundycattle629

I tried posting this question before, but I didn't get a greatanswer. Ãâ Please this is for the ANION test lab NOT the CATIONtest. Ãâ Thank you!

The lab is for CHEM II and it is taken out of a lab paq. Ãâ Beloware the materials used. Ãâ

Classify your ions according to the following three groups.

Several of the cations belong to more

than one group.

Group 1: Anions that WILL NOT PRECIPITATE in the presence of

silver nitrate.

Group 2: Anions that WILL PRECIPITATE in the presence of silver

nitrate and the resulting

precipitates WILL DISSOLVE upon acidification with nitric

acid.

Group 3: Anions that WILL PRECIPITATE in the presence of silver

nitrate and the resulting

precipitates WILL NOT DISSOLVE upon acidification with nitric

acid.

A. Write a net ionic equation for any reaction that produces a

precipitate.

B. Identify the anions that produce gas upon addition of

HCl.

C. Identify the anions that do not precipitate with silver

nitrate.

D. Identify the anions that react with silver nitrate to form

precipitates that dissolve when

acidified with nitric acid.

E. Identify the anions that react with silver nitrate to form

precipitates that do not dissolve when

acidified with nitric acid.

F. What simple test (other than a specific confirmation test)

would distinguish between CO3 2-

and NO3 - ?

Here are the materials we used

1 Ammonium Molybdate, 0.2 M - 2 mL in Pipet

1 Aqueous Ammonia, 6 M, NH4OH - 4 mL in Pipet

1 Barium Chloride, 0.3 M - 2 mL in Pipet

1 Hydrochloric Acid, 6 M - 8 mL in Dropper Bottle

1 Nitric Acid, 6 M - 2.5 mL in Pipet

1 Organic Reagent - 1.5 mL in Vial

2 Pipet, Empty Short Stem

1 Silver Nitrate, 0.1 N - 6 mL in White Dropper

Bottle

1 Sodium Bromide, 0.1 M - 2.5 mL in Pipet

1 Sodium Carbonate, 0.25 M - 2.5 mL in Pipet

1 Sodium Chloride, 0.1 M - 2.5 mL in Pipet

1 Sodium Iodide, 0.1 M - 2.5 mL in Pipet

1 Sodium Phosphate, 0.1 M - 2.5 mL in Pipet

1 Sodium Sulfate, 0.1 M - 2.5 mL in Pipet

1 Sodium Sulfide, 0.1 M - 2.5 mL in Pipet

1 Unknown - 5 mL in Pipet

Weekly leaderboard

Home

Homework Help 3,900,000

Chemistry 830,000

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard