Q: Indicate the direction of the equilibrium of the following.
A: In the given reaction a transfer of protons takes place. An acid gives a proton and a base accepts a…
Q: What is the difference betwween the strength of base of and concentration base
A: The strength of a base refers to how much of the base ions are released in a solution. It measures…
Q: For a triprotic weak acid, proof that, K = K1, K2, K3 [All equilibria reaction equations and…
A: The solution is as follows:
Q: To neutralize an acid, you must add of base. O a lower molar quantity O an equal molar quantity O a…
A: The neutralization reaction which includes that an acid react with a base (or vice-versa)…
Q: ______________contribute hydrogen ions (H+) to a solutionc. Acidsd. Compoundsa. Bases b. Isotopes
A: Acids are the chemical species that gives protons. or acids are the chemical species that are…
Q: sible arrow pointing in opposite directions en a compound is NOT completely ionized acid or a base…
A: Answer- Ionic equilibrium is denoted by sign of of reversibility so option 1 is true. Ionic…
Q: At equilibrium, ammonia in water is affected by which salt?
A: At equilibrium NH3 + H2O = NH4+ + OH-
Q: If the concentration of H3O^+ is 1.0x10^-13, the pH is?
A:
Q: Which of the following values will yield the weakest type of acid in the dissociation of an acid? *
A: Answer = 1.2 x 10-2
Q: A solution of HA, a weak acid (K = 0.0040), is prepared with a concentration of 0.579 M. Determine…
A: Given Data : 1. Ka =0.0040 2. Concentration of HA = 0.579 M
Q: A species that can either accept or donate a proton is called
A: Some substance have both properties i.e they can donate proton as well as accept proton.
Q: Which of the following is the strongest acid?
A: The organic compound in which more stable resonance structure is formed then the more stable…
Q: how do you calculate the concentration of hydronium in an acid equilibrium
A: pH = - log [H3O+] this is formula for find ph [H3O+] = 10-ph or [H3O+] = antilog (- pH)
Q: For each of the following compounds, identify the major species in solution and write a balanced…
A: An acid or base when in water gets ionized into anionic and cationic species. A strong acid/base…
Q: concentration:
A:
Q: Calculate the pH for the following weak acid. A solution of HCOOH has 0.21 M HCOOH at equilibrium.…
A:
Q: In the laboratory, a general chemistry student measured the pH of a 0.577 M aqueous solution of…
A:
Q: Which below is the proper equation(s) for ionization of acetic acid? a) CH3COOH…
A: Acetic acid (CH3COOH) is a weak acid. Weak Acids are those acids which are partially dissociate in…
Q: At what volume of added acid is the pH calculated by working an equilibrium problem based on the…
A: The titration curve given is,
Q: . Calculate the K, for the acid:
A:
Q: Complete the following Brønsted-Lowry reaction: H2O + CO2 > Acid Base
A: According to the Brønsted-Lowry concept, A compound which donates a proton to another compound is…
Q: Which compound(s) functions as a Brønsted-Lowry acid?
A: According to Bronsted-Lowry, a substance that donates the H+ (hydrogen ion) or proton is known as…
Q: Predict the of the acid-base equilibrium. Be sure to be able to explain why. HOʻ + HO Starting…
A: in the given acid-base equilibrium, we will use the concept of acidity to predict the equillibrium.
Q: For the reaction of C5H5N with water, write the base ionization constant expression.
A: we have to write the expression for base ionization constant for reaction of C5H5N with water
Q: At equilibrium, the value of [H+] in a 0.260M solution of an unknown acid is 0.00416M . Determine…
A: For acid HA, the acid dissociation constant Ka can be written as:
Q: A small amount of sodium hydroxide is added to water. When the chemical reaction reaches…
A: pH + pOH = 14 So, pOH = 14 - pH
Q: When sodium acetate is added to a solution containing sodium citrate, the equilibrium will shift to…
A: Sodium acetate is a basic salt as it formed from a strong base Sodium hydroxide and a weak acid…
Q: A0.148 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid…
A: Record the given data, A 0.148M solution of a monoprotic acid has a percent dissociation of 1.55%.…
Q: rder these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine…
A: The question is based on the concept of acidity. we have to arrange the given molecules according to…
Q: determine the K, for this acid.
A: Given :- pH = 5.098 concentration of phenol = 0.597 M To calculate :- Ka
Q: Which of the following solutions will h
A: the solutions which resists change in pH by the addition of small amount of strong acid (or) base…
Q: N(aq), was determined to have a p its hase ionization constant
A: According to the question, solution containing 4.2 g/L of the weak base pyridine was determined to…
Q: A buffer is needed to maintain a pH = 3.84. Of the acids listed in the table in the directions,…
A: Acetic acid
Q: You will find it useful to keep in mind that HF is a weak acid. acids: O 0.19 mol of KOH is added to…
A: Buffer contains HF and KF salt of weak acid.When KOH solution is added, assuming with no change…
Q: A species that can either accept or donate a proton is referred to as
A: A species that can either accept or donate a proton is referred to as what has to be given.
Q: In the laboratory, a general chemistry student measured the pH of a 0.455 M aqueous solution of…
A:
Q: Which of the following is true regarding acids and bases? a. All Bronsted-Lowry bases are…
A: Bronsted Acid-Base theory :- A bronsted acid is donate H+ ions and a base is that which accept that…
Q: When is it safe to assume that the change from initial concentration (+/- x) is small enough to be…
A: When % of dissociation of weak acid or base is very small then the change from initial concentration…
Q: Given: A solution contains 10−4 M total OCl species (TOTOCl), *90% of which is present as HOCl*…
A: The solution contains a total 10-4 M species of OCl out of which 90% is HOCl. To find: pH of the…
Q: hany moles of sodium sulfate will form if you fculfuris acid?
A: Mole is the amount of substance that have same number of atoms, molecules or ions as in the sample…
Q: HF is a weak acid, whose conjugate base is F-. Write the reaction that corresponds to Ka and Kb for…
A:
Q: Based on the principles of chemcial equilibriumm, how should the percent ionization vary as the…
A: Answer For a solution of a weak acid or a weak base, the percent…
Q: In the laboratory a student measures the percent ionization of a 0.453 M solution of acetic acid to…
A: Given that the conc. of acetic acid HA= 0.453 M percent ionization = 0.609 % The dissociation of…
Q: What is the importance of knowing the pH level of a substance?
A: pH means potential of Hydrogen. pH is an important quantity that reflects the chemical conditions of…
Q: Which of the following is the stronger acid?
A: The acid which easily donates H+ ion in the solution is the stronger acid.
Q: contains
A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid
Q: What is the value of K.
A: A + B = C + D (reaction at equilibrium) Kc = [product]/[reactant] Kc = [C].[D]/[A].[B] Where…
Q: A certain aquecus lQade monoprotic acid has a PH Of 3.0el for a 036z m solution.calaulate the acid…
A: Given : pH of solution = 3.61 concentration of acid solution = 0.362 M To calculate :- acid…
Q: An aqueous solution of ________ will produce an acidic solution. Sr(ClO4)2 LiBr LiNO2 NH4NO3 KNO3
A: An aqueous solution of a salt that is formed from a strong acid and a weak base will be acidic.
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- At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]
- In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
- The equilibrium between nitrogen monoxide, oxygen, and nitrogen dioxide may be expressed in the equation 2NO(g)+O2(g)2NO(g). Write the equilibrium constant expression for this equation. Then express the same equilibrium in at least two other ways, and write the equilibrium constant expression for each. Are the constants numerically equal? Cite some evidence to support your answer. Nitrogen monoxide and oxygen, both colorless gases, react to form reddish-brown nitrogen dioxide.The atmosphere consists of about 80% N2 and 20% O2, yet there are many oxides of nitrogen that are stable and can be isolated in the laboratory. (a) Is the atmosphere at chemical equilibrium with respect to forming NO? (b) If not, why doesnt NO form? If so, how is it that NO can be made and kept in the laboratory for long periods?What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.
- Write equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations. (a) 2 H2O2(g) 2 H2O(g) + O2(g) (b) CO(g) + O2g CO2(g) (c) C(s) + CO2(g) 2 CO(g) (d) NiO(s) + CO(g) Ni(s) + CO2(g)Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.The following two diagrams represent the composition of an equilibrium mixture for the reaction A2 + B2 2AB at two different temperatures. Based on the diagrams, is the chemical reaction endothermic or exothermic? Explain your answer using Le Chteliers principle. (A atoms are red and B atoms are green in the diagrams.)