Write balanced net ionic equation for the following reaction: HBr(aq)+Ca(OH)2(aq)→?
The net ionic equation is either H+(aq) + OH-(aq) ===> H2O(l) or 2H+(aq) + 2OH-(aq) ===> 2H2O(l) The first equation expresses lowest coefficients. The second equation expresses that there are indeed 2H+ and 2OH- in the original equation. Would you do me the favor of e-mailing me what is the correct answer? I'd like to be able to help others more completely.
How do you write the net ionic equation, including the phases for the following chemical reaction?
2HBr(aq)+Ba(OH)2(aq)-->2H2O(l)+BaBr2(aq) The equation is balanced, so write out the ions (remember to keep molecules intact): (2H+)+(2Br-)+(Ba+2)+(2OH-)-->(2H2O)+(Ba... Cancel out spectator ions. These are ions that watch the reaction without changing. For this problem Ba+2 & 2Br- are the spectator ions. You are left with the net ionic equation of… 2H+(aq)+2OH-(aq)-->2H2O(l)
Write the balanced net ionic equation, including the phases, for the following reaction:?
1. complete reaction:2 HCl(aq) + Ca(OH)₂ (aq) → CaCl₂ + H₂O (l) however since calcium chloride is soluble in water, there will be no observable reaction without boiling away the water. 2. net ionic equation: 2 H⁺(aq) + 2 Cl⁻(aq) + Ca⁺²(aq) + 2 OH⁻(aq) → Ca⁺²(aq) + 2 Cl⁻(aq)
Enter the balanced net ionic equation including phases for this reaction.?
AX + BY = AY + BX Na2SO4 + Ba(NO3)2 = 2Na(NO3) + BaSO4 molecular ecuation ((Na2)1+) + ((SO4)2-) + ((Ba)1+) +((NO3)2)1+ = (2(Na)1+) + ((NO3)1+) + (BaSO4)0 ionic equation ((SO4)2-) + ((Ba)1+) = (BaSO4)0 net ionic equation
What is a balanced chemical equation for the reaction between sodium and water?
Reaction of sodium with waterSodium metal reacts rapidly with water to form a colourless solution of sodium hydroxide (NaOH) and hydrogen gas (H2). The resulting solution is basic because of the dissolved hydroxide. The reaction is exothermic. During the reaction, the sodium metal may well become so hot that it catches fire and burns with a characteristic orange colour. The reaction is slower than that of potassium (immediately below sodium in the periodic table), but faster than that of lithium (immediately above sodium in the periodic table).2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
Write the balanced net ionic equation?
Chapter 4, Question 40 Write the balanced net ionic equation for each of these precipitation reactions. Enter the cation in the first box and the anion in the second box, with coefficients (if needed, leave 1s off as they are implied). Put charges in parentheses (charge multiple, if any, followed by sign) and phase in parentheses, e.g., Al3+(aq) should be entered as Al(3+)(aq). Also, identify the spectator ions. LiCl(aq) + AgNO3(aq) ? Correct. Write the net ionic equation for the reaction. Don't forget phase labels. Ag(+)(aq) + Cl(-)(aq) AgCl(s) Correct. Identify the spectator cation. Don't forget phase label. Li(+)(aq) Correct. Identify the spectator anion. Don't forget phase label. NO3(-)(aq) MgSO4(aq) + Na3PO4(aq) ? Correct. Write the net ionic equation for the reaction. 3Mg(2+)(aq) + 2PO4(3-)(aq) Mg3(PO4)2(s) Correct. Identify the spectator cation. Na(+)(aq) Correct. Identify the spectator anion. SO4(2-)(aq) Ba(OH)2(aq) + Na2SO4(aq) ? Correct. Write the net ionic equation for the reaction. Ba(2+)(aq) + SO4(2-)(aq) BaSO4(s) Correct. Identify the spectator cation. Na(+)(aq) Correct. Identify the spectator anion. OH(-)(aq) AlCl3(aq) + KOH(aq) ? Correct. Write the net ionic equation for the reaction. Al(3+)(aq) + 3OH(-)(aq) Al(OH)3(s) Correct. Identify the spectator cation. K(+)(aq) Correct. Identify the spectator anion. Cl(-)(aq)
Write the net ionic equation including the phases?
Everything the above answer says is true except the context being used for HClO2. This is a chlorus acid and it is not under the clssification for strong acids, there are 7 strong acids: HCl, hydrochloric acid; HBr hydrobromic acid; HI, Hydroiodic acid; HClO3 Chloric acid; HClO4 Perchlroric Acid, HNO3 Nitric acid; H2SO4 Sulfuric acid. and other 8 strong bases. the rest are weak acids, and weak bases. So therefore here HClO2 is a weak acid and tus a weak electrolyte. Learn this rule *Only strong electrolytes should be wrtten as individual ions(cations & anions) in an ionic equation. Thus the complete Ionic Equation is: HClO2(aq) + Na^+(aq) + OH^-(aq) ---> H2O(l) + ClO2^-(aq). Then cancel the *spectator ion or ions(the molecules, ions shown exactly alike on both sides cancel out just like in algebraic equations for those who are mathematically oriented). In this case is only Na^+. We are left with a Net Ionic Equation of: HClO2(aq) + OH^-(aq) ---> H2O(l) + ClO2-(aq).
Balanced Ionic and Net Ionic Equation?
(A) Among the alkaline earth metals you can chose the soluble salts of calcium, strontium or barium as one of the reactants, because the sulfates of these salts are slightly soluble. The least soluble one is barium sulfate and suppose we choose it as the product. All nitrates of metals are soluble, therefore we can choose barium nitrate as the reactant. Formula equation; Ba(NO3)2(aq) + H2SO4(aq) -------> BaSO4(s) + 2HNO3(aq) Ionic equation: Ba^2+(aq) + 2NO3^-(aq) + 2H^+(aq) + SO4^2-(aq) -------> BaSO4(s) + 2H^+(aq) + 2NO3^-(aq) Net ionic equation: (obtained by eliminating the spectator ions from both sides) Ba^2+(aq) + SO4^2-(aq) -------> BaSO4(aq) (B) Activity of halogens decreases from top to bottom within the group ( F > Cl > Br > I ) In the elemental state all halogens are diatomic molecules. F2 and Cl2 are gases, Br2 is liquid and I2 is solid. F2 replaces all other halogens. Cl2 replaces Br2 and I2. Br2 can only replace I2. Since I2 is the least active one it cannot replace any halogen. Formula equation; Cl2(g) + 2NaBr(aq) -------> 2NaCl(aq) + Br2(l) (note: all salts of sodium, potassium and ammonium are soluble) Ionic equation: Cl2(g) + 2Na^+(aq) + 2Br^-(aq) ------> 2Na^+(aq) + 2Cl^- (aq) + Br2(l) Net ionic equation: Cl2(g) + 2Br^-(aq) ------>2Cl^- (aq) + Br2(l) As it is clearly seen from the net ionic equation, Cl2 is reduced from 0 to -1 and Br^- is oxidized from -1 to 0.
Balanced Net Ionic Equations?
2Fe+3(aq) + 3S-2(aq) -> Fe2S3(s)
How do I write a balanced equation for Mg + O2?
Begin by familiarizing yourself with the two atoms' ionic charges.Magnesium, in Group IIA, has an ionic charge of 2+. (2 valence electrons lost when ionized) Oxygen, in Group 16A, has an ionic charge of -2 (2 Valence electrons gained when ionized).Knowing this, the ratio of the charges will be 1:1 in the resulting ionic compounds.Using the law of conservation of mass, #atoms before = #atoms after. (Matter is neither created nor destroyed) So, since Oxygen is diatomic (O2), all oxygen atoms in the products must be a multiple of 2. Using this known multiple, applying the 1:1 ratio to the equation means that 2 Magnesium atoms will be required to balance the charges of the two oxygen atoms. These 2 Magnesium atoms and O2 in the reactants looks like this:2 Mg + O2 -> ?Now, since there are two atoms of each, the resulting synthesis reaction will create two moles of MgO:2 Mg + O2 -> 2 MgOVerifying that it follows the law of conservation of mass, both the reactants and products contain 2 atoms of Mg and O.