what is the 1. chemical equation 2. complete ionic equation 3. net ionic equation include phase of HCH3COO+NaHCO3 pls correct my answers
1. CH3COOH(aq)+NaHCO3(aq)+CH3COONa(aq)+H2O(l)+CO2(g)
2. CH3COOH(aq)+OH-(aq)=CH3COO-(aq)+H2O(l)
3. OH(aq)+CO2(g)
The complete molecular equation is correct if you take away the + sign and replace it with an arrow where the arrow should be.
2. The complete ionic equation is not right. It should be this way.
CH3COOH(aq) + Na^+(aq) + HCO3^-(aq) ==> CH3COO^-(aq) + Na^+(aq) + H2O()l) + CO3(g). All I've done is taken your molecular equation #1 and split each reactant/product into ions if they ionize.
3. Cancel the spectator ions (those that appear on both sides of the equation) and you're left with the net ionic equation.
CH3COOH(aq) + HCOL3^-(aq) ==> H2O(l) _ CO2(g) + CH3COO^-(aq)
1. H2SO4 + 2NaHCO3= NaSO4 + 2CO2 + 2H2O
2. 2Na^+ + CO3^2- + 2H^+ SO4^2-= 2Na^+ + SO4^2- + 2H2O + 2CO2
3.HCO3^- + H^+ = H2O + CO2
1. The chemical equation for the reaction between acetic acid (CH3COOH) and sodium bicarbonate (NaHCO3) is correct:
CH3COOH(aq) + NaHCO3(aq) → CH3COONa(aq) + H2O(l) + CO2(g)
2. The complete ionic equation includes the dissociation of the compounds into their respective ions. However, acetic acid is a weak acid and does not fully dissociate in water. Sodium bicarbonate, on the other hand, is a salt and completely dissociates. Therefore, the correct complete ionic equation is:
CH3COOH(aq) + Na+(aq) + HCO3-(aq) → CH3COO-(aq) + Na+(aq) + H2O(l) + CO2(g)
Note: The sodium ion (Na+) appears on both sides of the equation and can be canceled out.
3. The net ionic equation shows only the ions that are involved in the reaction, excluding spectator ions. In this case, the spectator ions are Na+ on both sides. The net ionic equation is:
HCO3-(aq) + H3O+(aq) → H2O(l) + CO2(g)
Note: Instead of OH-(aq) as mentioned in your response, the correct net ionic equation involves H3O+ (hydronium ion) because acetic acid is a weak acid and donates H+ ions to the solution to form H3O+ ions.
1. The first answer you provided is the correct chemical equation. It shows the balanced equation for the reaction between acetic acid (CH3COOH), sodium bicarbonate (NaHCO3), resulting in sodium acetate (CH3COONa), water (H2O), and carbon dioxide (CO2) as products. The "(aq)" indicates that the substances are in aqueous form, and the "(g)" indicates that carbon dioxide is in gaseous form.
2. The second answer you provided is incorrect. The complete ionic equation shows all the species present as ions in the reaction. To write the complete ionic equation, you need to break down all the soluble ionic compounds (strong electrolytes) into their respective ions. In this case, acetic acid (CH3COOH) is a weak acid, so it does not completely dissociate into ions in aqueous solution. Sodium hydroxide (NaOH) was not present in the original equation, but if it were, it would dissociate into sodium ions (Na+) and hydroxide ions (OH-).
Since your original equation does not involve sodium hydroxide, we can move on to writing the correct complete ionic equation. Assuming CH3COOH is in its molecular form, it should be written as:
CH3COOH(aq) + Na+(aq) + HCO3-(aq) → CH3COO-(aq) + Na+(aq) + H2O(l) + CO2(g)
In this equation, we separate the sodium ion (Na+) and bicarbonate ion (HCO3-) as they are the only two ions that are involved in the reaction.
3. The third answer you provided is also incorrect. The net ionic equation represents the simplified form of the reaction, focusing only on the species that undergo a change. To write the net ionic equation, we eliminate the spectator ions, which are the ions that are present on both sides of the equation and do not participate in the actual reaction.
Using the correct complete ionic equation from step 2, we can identify the spectator ions as Na+ because it appears on both sides of the equation. Therefore, the net ionic equation for the reaction is:
HCO3-(aq) → H2O(l) + CO2(g)
This equation represents the reaction involving the bicarbonate ion (HCO3-) producing water (H2O) and carbon dioxide (CO2).