Write a net ionic equation for the overall reaction that occurs when aqueous solutions of sodium hydroxide and sulfurous acid (H2SO3) are combined. Assume excess base. Use the pull-down boxes to specify states such as (aq) or (s). ________(aq or a or l or g) +___________(aq or a or l or g) ----> _________(aq or a or l or g) +___________(aq or a or l or g)

Write a net ionic equation for the overall reaction that occurs when aqueous solutions of sodium hydroxide and sulfurous acid (H2SO3) are combined. Assume excess base. Use the pull-down boxes to specify states such as (aq) or (s). __(aq or a or l or g) +_(aq or a or l or g) ----> _(aq or a or l or g) +_______(aq or a or l or g)

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section: Chapter Questions

Problem 79A: Common Acids and Bases Use the data in Table 18.8 to answer the following questions. Which substance...

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Calculate the concentration of the following, aqueous solutions. Give your final answer to two decimal places. Hydroxonium ions, H3O+, in a solution of pH 6.4 Calcium hydroxide, Ca(OH)2 in a solution of pH 11.5 Use the ‘oxidation number method’ and balance the unfinished, ionic equation below. SO2 (aq) + IO3- (aq) → SO42- (aq) + I- (aq) Describe how a mixture of pentanoic acid (CH3CH2CH2CH2COOH) and potassium pentanoate (CH3CH2CH2CH2COOK) in solution can act as a buffer solution.
Use the following atomic masses (in g/mol): Mg = 24.31; O = 16; Ca = 40.08; C = 12.01; Na = 23; H = 1; N = 14.01; S = 32.06; Cl = 35.45; 4.) Sulfamic Acid (H3NSO3) is a monoprotic acid that can be used to standardize NaOH. Compute for the M of NaOH if 34.26mL is equivalent to 0.3337g sulfamic acid.
Common Acids and Bases Use the data in Table 18.8 to answer the following questions. Which substance is the most basic? Which substance is closest to neutral? Which has a concentration of H+=4.01010M ? Which has a pOH of 11.0? How many times more basic is antacid than blood?
For the following reaction, predict the products, write the total ionic equation and the net ionic equation: Ba(OH)2(aq) + H3PO4(aq) ⇄Total Ionic:Net Ionic: For the reaction below, predict the products, identify the acid, base, conjugate acid and conjugate base.H3O+(aq) + SO42-(aq) ⇄ A reaction is performed where 10.0 g K2S(s) are added to 250.0 mL of a 0.855 M HCl (aq) solution. Write a balanced equation for the reaction that would occur. Calculate the maximum number of moles of the gaseous product that can form? Which substance is the limiting reactant? How many moles of the non-limiting (or excess) reactant remain if the reaction goes to completion?What is the volume of the gas that forms if it is collected at 0.987 atm and 27.5°C?
What will be the pH of a solution created from a 10-fold dilution of a 0.50 M HNO3 solution? -0.30 -1.00 -1.30 -0.50
Calculate the pKa of hydrofluoric acid (HF(aq)) and hydrogen cyanide (HCN). What would be the pH of a solution containing 5 mM HF? What would be the pH of a solution containing 5 mM HCN?You do not need concentrations. Standard Gribbs Free energy for HF is -296.8 and for HCN is 124.7 This calculation assumes the acid is completely dissociated. You need the pKa to figure out how much of the H+ is free. This was all I was given. I do not know where to start, what I need, or what I need to calculate first. There are no other instructions or parts to this question. I'm at a loss, where do I begin?
Write the net ionic equation and eliminate spectator ions: a) Identify the following and acids or bases: HClO2 , C6H5NH2 ,CH3NH2 , C5H5N , C6H5CHCOOH , CH3CH2COOH. b) Write dissociation reactions for the molecules above, label the conjugate base/acid pairs. Write the equilibrium expression for all 6 reactions ( Ka or Kb) Make sure to balance. Did all your acids make H3O+ and all your bases make OH?
Question 11 Calculate the pH of mixing 90 mL of 0.19 mol/L hydrazine (H2NNH2) with 80 mL of a 0.14 mol/L H2NNH3Br solution. After determining the pH, again determine the pH of this same solution if 6.50 mL of 0.300 mol/L HNO3 is added.Give both answers to at least 3 decimal places.
YOU DON'T NEED TO ANSWER ALL THE QUESTIONS ALL I NEED HELP WITH IS QUESTIONS 4 and 5. I got d, e, e for the 1st 3 questions if that helps you, but you don't need to worry about questions 1-3 I just included them in case it helps you. 1.What reagent is used as the indicator for the neutralization? a)citric acid b)sodium hydroxide c)sodium citrate d)phenolphthalein 2. What is the mole ratio of NaOH to citric acid for this neutralization reaction? a)2 mole NaOH/1 mole citric acid b)1 mole NaOH/1 mole citric acid c)1 mole NaOH/2 mole citric acid d)1 mole NaOH/3 mole citric acid e)3 mole NaOH/1 mole citric acid 3.If 35.00 mL of 0.1104 M NaOH were used to reach the neutralization point, how many moles of NaOH were dispensed? a)3.154 x 10-3 mol NaOH b)1.104 x 10-4 mol NaOH c)258.8 mol NaOH d)3.864 x 10-3 mol NaOH 4. Using the above mole ratio, convert the moles of NaOH in the previous question to moles of citric acid. a)1.288…
The dissociation of 0.15 M phosphoric acid is given by:H3PO4(aq) + H2O(l) ⇄ H2PO4^-(aq) + H3O^+(aq) Ka = 7.1 x 10-3 (at 25°C) H2PO4^-(aq) + H2O(l) ⇄ HPO4^2-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) HPO4^2-(aq) + H2O(l) ⇄ PO4^3-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) A. Classify the species, H3PO4, H2PO4-, HPO4^2-, PO4^3-, as acid, base, or ampholyte.B. Applying the systematic method in solving acid-base equilibria problems, calculate the pH of the following:a. 0.050 M H3PO4 b. 0.050 M NaH2PO4 c. 0.050 M Na2HPO4d. 0.050 M Na3PO4
The dissociation of 0.15 M phosphoric acid is given by: H3PO4(aq) + H2O(l) ⇄ H2PO4^-(aq) + H3O^+(aq) Ka = 7.1 x 10-3 (at 25°C) H2PO4^-(aq) + H2O(l) ⇄ HPO4^2-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) HPO4^2-(aq) + H2O(l) ⇄ PO4^3-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) B. Applying the systematic method in solving acid-base equilibria problems, calculate the pH of the following: a. 0.050 M H3PO4 b. 0.050 M NaH2PO4 c. 0.050 M Na2HPO4 d. 0.050 M Na3PO4
What is the pOH for a solution at 25 °C that has a H3O+ concentration of 6.57 ×10-6 M? A 34.1 % (NH4 )2SO4 (molar mass = 132.1 g mol−1) has a density of 1.15 g mL−1. What is the molarity of this solution? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Determine the boiling point of a solution that contains 78.5 g of compound W (molar mass = 132.5 g mol–1) dissolved in 1088.6 g benzene (C6H6; molar mass = 84.156 g mol–1; Kb = 2.53 °C m–1; boiling point of pure benzene = 80.1 °C). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) NEED HELP ASAP NO WORK NEEDED