What is the Ionic equation for the reaction between calcium carbonate and hydrochloric acid?
Calcium carbonate dissolves into Ca(2+) and carbonate (CO3)(2-) ions. Hydrochloric acid dissolves into H(+) and Cl(-). When Ca(2+) and Cl(-) form CaCl2, it dissolves again (it is very soluble.) When H(+) combines with carbonate (CO3)(2-), you get a mix of ions, but if you have enough acid, you primarily get H2CO3, carbonic acid. This decomposes into H2O liquid and CO2 gas, which is what happens in your soda when you open it and relieve the pressure—it makes bubbles of CO2. Since CaCl2 is soluble, Ca(2+) and Cl(-) are spectator ions. You can cancel them out of the total reaction to get the net ionic equation. The net equation is then 2H(+) +CO3(2-) → H2O (liquid) and CO2 (gas).
Help with net ionic equations? (gas-forming reactions)?
1. Write a net ionic equation for the reaction that occurs when excess hydrobromic acid (aq) and zinc carbonate (s) are combined. 2. Write a net ionic equation for the reaction that occurs when potassium sulfide and excess hydroiodic acid are combined. 3. Write a net ionic equation for the reaction that occurs when calcium sulfite (s) and excess hydrochloric acid (aq) are combined. Note: Sulfites follow the same solubility trends as sulfates.
Predicting products of gas formation reactions?
The reaction of an acid with a carbonate or bicarbonate will always produce CO2 gas. HCl(aq) + NaHCO3(s) --> NaCl(aq) + CO2(g) + H2O(l) The net ionic equation is H+ + NaHCO3(s) <==> Na+ + CO2(g) + H2O 2HCl(aq) + Na2CO3(s) --> 2NaCl(aq) + CO2(g) + H2O(l) The net ionic equation is 2H+ + Na2CO3(s) --> 2Na+ + CO2(g) + H2O(l) HCl (aq) + NaOH (aq) ---> NaCl(aq) + H2O(l) .... of course, this is double replacement. Water is the "insoluble" precipitate. The net ionic eqution is H+ + OH- --> H2O(l) HCl (aq) + NaC2H3O2 (aq) ---> HC2H3O2(aq) + NaCl(aq) .... this reaction forms molecular acetic acid. Acetic acid is a weak acid and does not dissociate very much. we would write the net ionic equation as H+ + C2H3O2^- <==> HC2H3O2(aq) =============== Follow up ================ A few corrections to Halchemist's otherwise useful response. There is no H2CO3 formed in the first place to later decompose. Halchemist wrote, ....H+(aq) + HCO3- ------> CO2(g) + H2O(l) ....2H+(aq) + CO3=(aq) -------> CO2(g) + H2O(l) While a small point, these are not actually the net ionic equations if NaHCO3 and Na2CO3 are both solids initially. The net ionic equation includes the substances as they actually are. See my answer above. Also, be sure to indicate the equilibrium that is established when hydrogen ion reacts with acetate ion, as in H+ + C2H3O2^- <==> HC2H3O2(aq)
Question about net ionic reaction with a gas forming reaction?
I do not know that it is conventional to use H3O+ in ionic or net ionic equations - this is the first time in many years of chemistry that I have seen this done . Keep things simple I say: Let us work out from the beginning: Molecular equation: MgCO3(s) + 2HCl(aq) → MgCl2(aq) + CO2 (g) + H2O(l) Full ionic equation: MgCO3(s) + 2H+(aq) + 2Cl-(aq) → Mg2+(aq) + 2Cl-(aq) + CO2(g) + H2O(l) Net ionic equation: MgCO3(s) + 2H+(aq) → Mg2+(aq) + CO2(g) + H2O(l) In my opinion this is the correct way of presentation for all three equations: Some notes and explanations: If the writer wishes to have as the FULL IONIC equation: MgCO3(s) + 2H3O+(aq) + 2Cl-(aq) → etc Then he cannot have as the molecular equation: MgCO3(s) + 2HCl(aq) → etc Where does the water come from to make H+ into H3O+? He would have to write MgCO3(s) + 2HCl(aq) + 2H2O Then he can write as full ionic equation: MgCO3(s) + 2H3O-(aq) + 2Cl-(aq) Then he would have to write as the net ionic equation: MgCO3(s) + 2H3O+(aq) → Mg2+(aq) + CO2(g) + 3H2O(l) Check the answer in the book: On the left side he has 6H , but on the right he has only 4H so the equation is not balanced . I think that the writer is trying to be too clever by introducing H3O+ into the equation , instead of sticking with convention and showing only H+. As a result he has made a number of mistakes.
Net Ionic Equation - Any help is appreciated!!?
Write the net-ionic equation for the following reactions: Include phase labels for products. Also classify each reaction type (i.e acid-base, acid-base with gas formation, precipitate, or redox) a) HNO3 (aq) + KOH (aq) --> KNO3 + H2O b) 2Na(s) + 2H2O(l) ---> 2NaOH + H2 c) 2HC2H3O2 (aq) + Ba(OH)2 (aq) --> Ba(C2H3O2)2 + 2H2O d) 2Li(s) + Cu(NO3)2 (aq) --> 2LiNO3 + Cu
Net ionic equations....plzzz help chemistry problem?
MgCO3 (s) + 2 HClO4 (aq) -----> Mg(ClO4)2 (aq) + H2O (l) + CO2 (g) CO3 2- (s) + 2 H+ (aq) ----> H2O (l) + CO2 (g) ....the only items changing phase are the ones in then net ionic equation.
What is the balanced net-ionic equation for the gas producing reaction between hydrobromic acid and solid calcium carbonate?
The steps for writing a net ionic equation:If the reaction is given in sentence form, convert reactants to formulas, and impute products. This takes some prior knowledge of nomenclature and classifications of reaction types (e.g., here a double replacement with subsequent gas formation).Balance this molecular equation.If the reaction is taking place in aqueous solution, any of the ionic reactants and products that are in solution and are fully dissociated should be written as the ions instead of molecules (because that’s what they will be in solution).Cancel any components that appear on both sides.Neaten up: rewrite the equation without the components you cancelled in step 4.Here’s how it should look as you progress through the steps:
What is a balanced equation of the reaction between hydrochloric acid and sodium carbonate?
2HCl + Na2CO3 → 2NaCl + H20 + CO2
How do I write a net ionic equation if the reactants and products are all aqueous?
How do I write a net ionic equation if the reactants and products are all aqueous?I’m going to take you at your word, that all the reactants and products are aqueous. So take this, as an for example:KCl (aq) + NaNO[math]_3[/math] (aq) → KNO[math]_3[/math] (aq) + NaCl (aq)To convert a balanced equation to a net ionic equation, you write the aqueous reactants and products as dissociated ions (if they are ionic, that is, no insoluble salts, gases, or weak electrolytes formed):K[math]^+[/math] (aq) + Cl[math]^-[/math] (aq) + Na[math]^+[/math] (aq) + NO[math]^-_3[/math] (aq) → K[math]^+[/math] (aq) + NO[math]^-_3[/math] (aq) + Na[math]^+[/math] (aq) + Cl[math]^-[/math] (aq)and then you cross out the ions that appear on both sides of the equation (the spectator ions). Once you’ve done that, you’re left withnuttin’ → nuttin’Meaning, it technical lingo, N.R. or no reaction. Adding an aqueous solution of potassium chloride to an aqueous solution of sodium nitrate causing nothing but a mixture of salts to form. No chemical reaction takes place.