No sure what I did wrong here. Maybe the net ionic equestion it not correct Write the balanced NET IONIC equation for the reaction that occurs when nitric acid and calcium hypochlorite are combined. It is not necessary toinclude states such as (aq) or (s).H (aq)ClO" (aq)HCIO (1)This reaction is classified as: Strong Acid + Weak BaseThe extent of this reaction is: 100%When 35.0 mL of 0.400 M nitric acid and 35.0 mL of 0.200 M calcium hypochlorite are combined, the pH of the resulting solution will beless thanV seven.

Formula for Nitric acid is HNO3 Calcium hypochlorite is Ca(ClO)2

Write the balanced NET IONIC equation for the reaction that occurs when nitric acid and calcium hypochlorite are combined. It is not necessary to include states such as (aq) or (s). H (aq) + CIO" (aq) HCIO (1) > This reaction is classified as: Strong Acid + Weak Base v The extent of this reaction is: 100% When 35.0 mL of 0.400 M nitric acid and 35.0 mL of 0.200 M calcium hypochlorite are combined, the pH of the resulting solution will be less than seven.

Write the balanced NET IONIC equation for the reaction that occurs when nitric acid and calcium hypochlorite are combined. It is not necessary to include states such as (aq) or (s). H (aq) + CIO" (aq) HCIO (1) > This reaction is classified as: Strong Acid + Weak Base v The extent of this reaction is: 100% When 35.0 mL of 0.400 M nitric acid and 35.0 mL of 0.200 M calcium hypochlorite are combined, the pH of the resulting solution will be less than seven.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 26P

See similar textbooks

Similar questions

Of the following, which has the greatest buffering capacity (aq., 25 oC)? A) 0.543 M NH3 and 0.555 M NH4ClB) 0.087 M NH3 and 0.088 M NH4Cl C) 0.234 M NH3 and 0.100 M NH4ClD) 0.100 M NH3 and 0.455 M NH4Cl E) They are all buffer solutions and would all have the same capacity.
During the titration of an HClO4 solution with 0.10320 M NaOH, a student, Lovely became distracted and overshot the endpoint. A fellow student Ashley suggested that he should record the present volume of NaOH added and titrate the excess with a standard acid solution. If the original sample volume was 25.000 mL, the volume of NaOH added was 28.060 mL. It took 3.4700 mL of 0.10940 M HCl to back-titrate the NaOH and calculate the molar concentration of the original HClO4
Consider the following acid base titration between H2C3H5O3 (aq) with KOH (aq). A)Write a complete balanced equation. B) If 25.0 mL of the acid required 13.6 mL of 0.0789 M of the base to reach the equivalence point, what is the concentration of the acid? C)Which of the reactant is the limiting reactant?
2.80 g of sodium acetate, CH3COONa was dissolved in 150.0 mL of water, H2O. A solution of 0.025 M ethanoic acid, CH3COOH was added into the above salt solution. Calculate the pH of the mixed solution. Pka=CH3COOH = 4.10, Molar mass of CH3COONa = 82.0 g mol-1
Write the balanced NET IONIC equation for the reaction that occurs when hydrochloric acid and calcium hypochlorite are combined. It is not necessary to include states such as (aq) or (s). This reaction is classified as: .The extent of this reaction is: .When 35.0 mL of 0.400 M hydrochloric acid and 35.0 mL of 0.200 M calcium hypochlorite are combined, the pH of the resulting solution will be seven. Submit Answer
determine the ph change when .061 mol HClO4 is added to 1 L of abuffer solution that is .305 Min HCN and .203 M in CN-
A pure organic compound has the formula C4H8SOx. A sample of a compound wasdecomposed; the sulfur was converted to sulfate and titrated in a modified version of theadsorption indicator procedure. From the following data, determine the correct formula forthe compound.Given: weight of sample = 12.64 mgBa(ClO4)2 needed for titration = 10.60 mL of 0.0100 M Ba(ClO4)2
Consider a buffer solution that consists of two separate components: the weak acid ch3coo aq), and its conjugate base, ch3coo (aq) (added as NaCH3COO A) which component will react with H+ from a strong acid? write the ionic equationvfor the reaction that occurs when H+ is added to the buffered solution. B) which component will react with oh- from a strong base? Write thebionic equation for the reaction that occurs when oh- is added to the buffered solution.
A buffer solution is made that is 0.488 M in H2CO3 and 0.488 M in KHCO3. If Ka1 for H2CO3 is 4.20x10^-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.124 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O^+ instead of H^+) + +
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction? Kc is the product of all reaction products (choose from: Multiplied by, added to, divided by, subtracted from) the product of the reactants, with all concentrations of reactants and products raised to their respective stoichiometric powers. As the titration proceeds, the amount of reactants (choose from: Increases, decreases, remains the same) and the amount of products (choose from: Increases, decreases, remains the same). Because the value of the numerator is (Choose from much greater than, much less than, approximately equal to) the value of the denominator, the value of Kc will be (Choose from much greater than, much less than, approximately equal to)1 for an effective titration reaction.
If Sn3(PO4)2 solution is to be subjected to argentometric titration, a) Write the balanced titration reaction. (products are Ag3PO4(s),, other ions are spectator ions b) Write the stoichiometric relationship (fundamental eqn) between the titrant (AgNO3) and the titrand (Sn3(PO4)2. c) Is this a feasible titration technique? Why?
How will the following sitations affect the final calculation of the molarity of HC2H3O2? The end point of the vinegar titration was surpassed. (excess NaOH was added.)