Nitric Acid + Calcium hydroxide ---> calcium nitrate + water

I wrote it as :

NO3 + Ca(OH)2 ---> Ca(NO3)2 + H20

Did I write it correctly? Where should I put my charges? I also have big time trouble balancing this one.

  1. 👍
  2. 👎
  3. 👁
  1. If you wrote it correctly you don't have any charges. Nitric acid is HNO3. That is a compound and has no charge. Same for Ca(OH)2, Ca(NO3)2, and H2O.

    1. 👍
    2. 👎
  2. This is getting really confusing for me. My teacher said that if its an ionic compound then it must have a charge in. On this sheet she gave me of common ions, hydroxide has a negative 1 charge. I also went back to some of the problems she did as an example in class, and she put charges on them. I have no idea what to do with these charges now. Like for Ca(OH)2 she put 2 charges on calcium and - 1 charge on OH. Then she put paranthesis around OH to make it 2 to match Ca.

    1. 👍
    2. 👎
  3. OK. You may be trying to write ionic equations. If so, then the HNO3 would be written as H^+ + NO3^-. The Ca(OH)2 [Ca ion is a +2 charge and OH is a -1 charge which accounts for the formula as it is] is only partially soluble in water and may be written Ca(OH)2(s), Ca(NO3)2 is ionic and in solution dissolves easily so it consists of Ca^+2 and 2NO3^-. The H2O is a liquid, and is largely unionized, so we write it as H2O(l).
    So the ionic equation would be written as
    H^+ + NO3^- + Ca(OH)2(s) ==> Ca^+2 + 2NO3^- + H2O
    I don't know how your teacher treats Ca(OH)2, s/he may have written it as Ca(OH)2(s), or as Ca(OH)2(aq), or as Ca^+2 + 2OH^-.
    Is this close to what you are trying to do?

    1. 👍
    2. 👎
  4. My teacher does not care that we put symbols as the end of our equations like (s) or (aq) but I think we are balancing ionic equations. But she puts +2 charge on Ca and -1 charge on OH

    She also puts charge +2 charge on Calcium on the product side and a -1 charge on the NO3 as well.

    For the final equation that I wrote (Unbalanced):

    HNO3 (H has +1 charge, NO has -1) + Ca(OH)2 (Ca has +2 charge, OH has -1) -------> Ca(NO3)2 (Ca +2 charge, NO -1 charge) + H2O

    That is what I wrote, would that be an ionic equation? Does that even look right? Also, I have trouble balanceing it.

    1. 👍
    2. 👎
  5. The way I have been taught is to go the easy route and write, and balance, the molecular equation. Here is the molecular equation.
    2HNO3 + Ca(OH)2 ==> Ca(NO3)2 + 2H2O

    The we make that into the ionic equation.
    The rules are to write those compounds that are ionic as ions, write solids, and unionized compounds as the molecule. Here we would have,

    2H^+ + 2NO3^- + Ca^+2 + 2OH^- ==> Ca^+2 + 2NO3^- + 2H2O.

    THEN, the next step is change this into a NET IONIC EQUATION. We do that by canceling ions common to both sides. In the above equation, We have Ca^+2 on both sides so cancel those. We have 2 NO3^- on both sides so cancel those. What's left?
    2H^+ + 2OH^- ==> 2H2O and that is the net ionic equation. That may be where your teacher is going in the end. To answer an earlier question, you put the charges on the ions when you move from the molecular equation to the ionic equation.

    1. 👍
    2. 👎
  6. Thanks bob. I think im going to ask my teacher about this. She probably made us put charges on them to help us because we just started doing it.

    1. 👍
    2. 👎
  7. I agree with DrBob's approach. There is a need to add in the phase symbols as this does enable the equation to make more sense.
    This experiment is usually done by dissolving solid Ca(OH)2 in nitric acid, other wise there is nothing to see.
    So I would start from
    2HNO3(aq) + Ca(OH)2(s) ==> Ca(NO3)2(aq) + 2H2O(l)

    then the ions for the (aq) species

    2H^+(aq) + 2NO3^-(aq) + Ca(OH)2(s)==> Ca^+2(aq) + 2NO3^-(aq) + 2H2O(l)

    losing the common ions

    2H^+(aq) + Ca(OH)2(s)==> Ca^+2(aq) + 2H2O(l)

    which is what would be expected for dissolving Ca(OH)2 in an acid.

    Does this help?

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Calabasas HS

    A 46.2-mL, 0.568 M calcium nitrate [Ca(NO3)2] solution is mixed with 80.5 mL of1.396 M calcium nitrate solution. calculate the concentration of the final solution

  2. chemistry(Urgent Please help)

    A student is asked to standardize a solution of barium hydroxide. He weighs out 0.945 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid). It requires 33.9 mL of barium hydroxide to reach the endpoint. A.

  3. Chemistry

    A beaker of nitric acid is neutralized with calcium hydroxide. Write a balanced molecular equation and a net ionic equation for his reaction

  4. Chem

    Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions are mixed. Include the physical states. A. nitric acid, HNO3 , and calcium hydroxide, Ca(OH)2 B. lead(II) nitrate, Pb(NO3)2 , and

  1. Chemistry

    Complete the following acid-base reaction with balanced molecular, total ionic and net ionic equations: calcium hydroxide (aq) + acetic acid (aq) ----> ? I know that calcium hydroxide is ca(OH)2 and that acetic acid is CH3COOH. I

  2. Chemistry

    a solution saturated in calcium hydroxide(limewater) has a pH of 12.35. What is Ksp for calcium hydroxide? How do i start this problem. please

  3. chemistry

    When 11.0 g of calcium metal is reacted with water, 5.00 g of calcium hydroxide is produced. Using the following balanced equation, calculate the percent yield for the reaction? Ca(s) + 2 H2O(l) → Ca(OH)2(aq) + H2(g) 84.0% 12.3%

  4. chemistry

    calcium hydroxide is titrated with nitric acid.What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 ml of 0.0500 M nitric acid?

  1. Chemistry

    The acid-base reaction between phosphoric acid, H3PO4, and calcium hydroxide, Ca(OH)2, yields water and calcium phosphate. For each mole of calcium phosphate produced by this reaction, how many moles of water are also produced?

  2. Chemistry

    Can calcium hydroxide solution be used to distinguish Co(NO3)2 and Fe(NO3)3 solutions using only the titration technique? Why or why not?

  3. Chemistry

    Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: A 2.00-g sample of is reacted with 1.93 g of . How many grams of water remain after the reaction is complete? 0.0714 1.29 0.00 1.04 0.00396

  4. Chemistry

    A Rolaids tablet contains calcium carbonate to neutralize stomach acid. One Rolaids tablet requires 44.55 mL of 0.448 M hydrochloric acid to convert its calcium carbonate into calcium chloride, carbon dioxide and water. How many

You can view more similar questions or ask a new question.