FUND.OF GEN CHEM CHAP 1-13 W/ACCESS
16th Edition
ISBN: 9781323406038
Author: McMurry
Publisher: PEARSON C
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 5, Problem 5.36AP
Write balanced ionic equations and net ionic equations for the following reactions:
(a) A precipitate of barium sulfate forms when aqueous solutions of barium nitrate and potassium sulfate are mixed.
(b) Zinc ion and hydrogen gas form when zinc metal reacts with aqueous sulfuric acid.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Complete the following precipitation reactions using balanced chemical equations:
Write a balanced equation for each of the following singlereplacement reactions. (a) Zinc granules are added to carbonic acid. (b) Cadmium metal is added to acetic acid.
75 mL of 0.300 mol/L sodium phosphate solution is combined with 67.5 mL of 0.350 mol/L calcium bicarbonate.
a)Before you begin your reaction, you must accurately produce 1.500 L of your sodium phosphate solution from sodium phosphate trihydrate solid. Write out a procedure to explain all the steps you will take in the lab when making the solution to ensure that your solution concentration is accurate. Please include calculations that show the required mass of solid. Also include the correct names of all equipment used.
b)You have a super powerful microscope in your lab! You are able to zoom in on your sodium phosphate solution and take a picture at the molecular level. Label the diagram on the left with the correct choices from the box on the right. You may use arrows or rewrite the symbols in one appropriate place.
c)In one sentence, explain what the diagram is showing.
Chapter 5 Solutions
FUND.OF GEN CHEM CHAP 1-13 W/ACCESS
Ch. 5.2 - Ozone (O3) is formed in the earths upper...Ch. 5.2 - Balance the following equations:...Ch. 5.2 - Prob. 5.3KCPCh. 5.3 - Many kidney stones are formed by precipitation of...Ch. 5.3 - Prob. 5.2CIAPCh. 5.3 - Predict the solubility of the following compounds:...Ch. 5.3 - Prob. 5.5PCh. 5.4 - Write and balance equations for the following...Ch. 5.5 - Prob. 5.7PCh. 5.5 - Prob. 5.8P
Ch. 5.5 - Prob. 5.9PCh. 5.6 - Prob. 5.3CIAPCh. 5.6 - The redox reaction that provides energy for the...Ch. 5.6 - Prob. 5.10PCh. 5.6 - Prob. 5.11PCh. 5.6 - For each of the reactions you identified as redox...Ch. 5.7 - Prob. 5.13PCh. 5.7 - Identify each of the tractions in Problem 5.13 as...Ch. 5.7 - For each traction in Problem 5.13 that you...Ch. 5 - Assume that the mixture of substances in drawing...Ch. 5 - Prob. 5.17UKCCh. 5 - Prob. 5.18UKCCh. 5 - Prob. 5.19UKCCh. 5 - Prob. 5.20UKCCh. 5 - Prob. 5.22APCh. 5 - Why is it not possible to balance an equation by...Ch. 5 - Write balanced equations for the following...Ch. 5 - Prob. 5.25APCh. 5 - Which of the following equations are balanced?...Ch. 5 - Prob. 5.27APCh. 5 - Balance the following equations:...Ch. 5 - Prob. 5.29APCh. 5 - When organic compounds are burned, they react with...Ch. 5 - Prob. 5.31APCh. 5 - Hydrofluoric acid (HF) is used to etch glass...Ch. 5 - Write a balanced equation for the reaction of...Ch. 5 - Identify each of the following reactions as a...Ch. 5 - Write balanced ionic equations and net ionic...Ch. 5 - Write balanced ionic equations and net ionic...Ch. 5 - Prob. 5.37APCh. 5 - Prob. 5.38APCh. 5 - Which of the following substances are likely to be...Ch. 5 - Which of the following substances are likely to be...Ch. 5 - Use the solubility guidelines in Section 5.3 to...Ch. 5 - Use the solubility guidelines in Section 5.3 to...Ch. 5 - Prob. 5.43APCh. 5 - Prob. 5.44APCh. 5 - Prob. 5.45APCh. 5 - Prob. 5.46APCh. 5 - Where in the periodic table are the best reducing...Ch. 5 - Prob. 5.48APCh. 5 - Prob. 5.49APCh. 5 - Prob. 5.50APCh. 5 - Prob. 5.51APCh. 5 - Assign an oxidation number to the metal in the...Ch. 5 - Prob. 5.53APCh. 5 - Which element is oxidized and which is reduced in...Ch. 5 - Prob. 5.55APCh. 5 - Prob. 5.56APCh. 5 - Prob. 5.57APCh. 5 - Identify the oxidizing agent and the reducing...Ch. 5 - Prob. 5.59CPCh. 5 - Prob. 5.60CPCh. 5 - Prob. 5.61CPCh. 5 - Prob. 5.62CPCh. 5 - Prob. 5.63CPCh. 5 - Prob. 5.64CPCh. 5 - Prob. 5.65CPCh. 5 - Prob. 5.66CPCh. 5 - Hard water contains magnesium and calcium ions...Ch. 5 - Prob. 5.68CPCh. 5 - Prob. 5.69CPCh. 5 - Prob. 5.70CPCh. 5 - Geologists identify carbonate minerals by reaction...Ch. 5 - Prob. 5.72CPCh. 5 - High temperature combustion processes, such as in...Ch. 5 - Milk of magnesia is an over-the-counter product...Ch. 5 - Prob. 5.75GP
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, biochemistry and related others by exploring similar questions and additional content below.Similar questions
- Consider the following reaction and its equilibrium constant: 12(g) 21(g) Kp = 0.209 atm A reaction mixture contains 0.89 atm 12 and 1.77 atm I. Which of the following statements is TRUE concerning this system?arrow_forwardCalculate the molarity of dilute Ca(OH)2 solution if the titration of 30.00 mL of 0.05231 M HCl required 24.76 mL of the acid. An 0.2500 g hydroxide tablet sample submitted in the lab used 36.75 mL during titration. How much is the hydroxide in mg present?arrow_forwardPepto-Bismol, an antacid and antidiarrheal, contains bismuth subsalicylate, C7H5BiO4. Some users of this product can experience a condition known as “black tongue,” which is caused by the reaction of bismuth(III) ions with traceamounts of S2- in saliva to form a black precipitate. Write the balanced net ionic equation for this precipitation reaction.arrow_forward
- A 100.0 mL sample of 0.200 M aqueous hydrochloric acid is added to 100.0 ml of 0.200 M aqueous ammonia in a calorimeter whose heat capacity (excluding any water) is 480.0 J/K. The following reaction occurs when the two solutions are mixed. HCl(aq)+NH,(aq)—NH_Cl(aq) The temperature increase is 2.34 °C. Calculate AH per mole of HCI and NH, reacted. Select one: о a. -1.96 KJ/mol b. 154 KJ/mol O c. 485 KJ/mol d. 1.96 KJ/mol Jm e. -154 J/molarrow_forwardConsider the following equilibrium at 298 K. R = 8.314 J/K-mol Citrate Isocitrate Using the equilibrium concentrations of [Citrate] = 2.15 M and [Isocitrate] = 0.00825 M, calculate K'g, then AG°. Which one of the following is the correct value for AG in units of kJ/mol? 5990 kJ/mol -2480 kJ/mol 2.48 kJ/mol 13.8 kJ/mol 5.99 kJ/mol -2.48 kJ/mol -5990 kJ/mol -9.99 kJ/mol -13800 kJ/mol 13800 kJ/mol -5.99 kJ/mol 9.99 kJ/mol 2480 kJ/mol 9990 kJ/mol -13.8 kJ/mol -9990 kJ/mol O O O O O O O O O O0000 O Oarrow_forwardThe main constituents in vinegar are water and ethanoic acid (CH3COOH). In order to determine the concentration of acid in homemade vinegar, a student titrated 25 cm3 of 001 M NaOH against the vinegar. The equation for the reaction is: CH3COOH(aq) + NaOH(aq) ® CH3COONa(aq) + H2O(l) The following titration results were obtained: Burette readings (cm3) Rough 1 2 Final burette reading 20.10 38.90 31.40 Initial burette reading 0.10 20.00 12.50 Volume of vinegar used 20.00 18.90 18.90 (a) What volume of vinegar should be used in the calculation? (b) What is the mole ratio of NaOH:CH3COOH? (c) Calculate the number of moles of alkali in 25 cm3 of NaOH solution used. (d) How many moles of acid were used in the titration? (e) Calculate the…arrow_forward
- Calculate the average charge of H3A+ at pH 5.10 (pKa = 2.1, 3.9, 9.8). (Hint: remember that the answer must be ± 0.5 of the dominant charge.)arrow_forwardGiven the equation below, determine which statement is incorrect. 4C(s) + 6H2(g) + O2(g) → 2C2H5OH(1) AH°=555.4 kJ A) If the equation above is multiplied by two, AH° = - 1110.8 kJ B) For every 0.5 mol of O2, AH° = -277.7 kJ If the state of ethanol changes from the liquid state to the gas state, the value for AH° no loner applies. D) The value of 571.1 kJ applies to one mole of liquid ethanol. E) If the equation above is reversed, AH° = + 555.4 kJarrow_forwardUse the Michaelis-Menten equation to determine the velocity of reaction when: • [S] = 15.0 mM Vmax = 94.0 umol/mL sec • Km = 4.00 mM Velocity of reaction = umol/mL secarrow_forward
- Complete the following table, which lists information about the measured acid dissociation constants of three unknown weak acids. Note: be sure each number you put in the table has the correct number of significant digits. acid K Κα PK relative strength a a ☐ x10 A B C 1.2 × 10 3. 10 4 ☐ 11.539 ×arrow_forwardThe following data give the constant dissociation, Ka (for acetic acid at various temperatures): T(°C) 0 Ка 1.657 x 10-5 10 1.729 x 10-5 15 1.745 x 10-5 25 1.753 × 10-5 kJ ΔΗ° = 1.53 mol Submit Previous Answers Part B Correct Plot Inka vs. 1/T and fit a line to the points. The slope will correspond to —▲H° / R. 1/T InKa 3.66 x 10-3-11.01 3.53 x 10-3-10.97 3.47 x 10-3-10.96 3.36 × 10-3-10.95 InKa = (−184 K) (±) — 10.3 = slope -184 K = AH° R AH° -184 K = 0.008314 kJ/(mol·K) AH 1.53 kJ/mol = Use these data, and the constant dissociation at 25 °C, to calculate AS° for acetic acid ionization. (InK Express your answer with the appropriate units. μÅ AS° = Value Units ? -AH° + ᎡᎢ. AS° Rarrow_forward(i) MnO is basic whereas Mn207 is acidic in nature. Why? (ii) Transition metals form alloys. Why? (iii) Complete the following equation: 2MnO4 + 4KOH + O2 ———>arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
GCSE Chemistry - Acids and Bases #34; Author: Cognito;https://www.youtube.com/watch?v=vt8fB3MFzLk;License: Standard youtube license