What is the concentration of free Ag+ in 3.7099e-4 M AgNO3 and 1.4440 M NaCN? Ag+ + 2 CN− → [Ag(CN)2]−

Q: An analytical chemist is titrating 94.8 mL of a 0.4000M solution of nitrous acid (HNO,) with a…

A: Given : Volume of HNO2 solution = 94.8 mL = 0.0948 L                                      (since 1 L…

Q: 8. The addition of acetic acid and ________ to water produces a buffer solution. A. HC2H3O2 B. KI…

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Q: What is the approximate value of the equilibrium concentration of A- for the mixture of 0.1 M HCI…

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Q: Milk of magnesia is a saturated solution of Mg(OH) 2 (Molar mass 58.32) which is soluble in water…

A: Given solubility in water = 9.62 mg/100 ml molar mass = 58.32 g/mol

Q: 5) The oxides and hydroxides of gallium exhibit both acidic and basic behaviors B) What is pCa for a…

A: Gallium metal is stable in dry air. It gradually oxidizes in moist air to form a protective film…

Q: Phosphoric acid is a triprotic acid (Kal 6.9 x 10-3, K2 = 6.2 × 10-8, and Ka3 = 4.8 x 10-13). To…

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Q: Calculate the [NH3] in a solution of 0.650 M ammonium fluoride (NH4F). Hint: Use the Ka of HF (6.8 x…

A: Equation for Ka of HF and Kb of NH3- HF aq ⇔H+aq + F-aqKa =H+F-HFNH3 aq⇔NH4+ aq+OH- aqKb =NH4+OH-NH3

Q: Complete the table relating the values of AG° and K. AG° K 1 = 0 > 0 Answer Bank > 1 < 1 = 1

A: ∆G° = Standard Gibbs Free Energy Change K = Equilibrium constant

Q: What is the solubility of silver oxide, in a solution buffered at pH 10.50? The equilibrium is…

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Q: Calculate the buffer capacity of a buffer solution prepared by mixing 0.215M sodium acetate and…

A: Given =  Concentration of sodium acetate  = 0.215M Conc of acetic acid =  0.125M pKa =  4.76

Q: A standardized iodine solution is used to titrate hydrazine sulfate in a sodium bicarbonate-…

A: This question is from redox titration where we apply the concept of equivalence to find the Molarity…

Q: What is the pH of a 1.2 M pyridine solution that has Kp = 1.9 x 10 9? The equation for the…

A: The concentration of pyridine = 1.2 M  Kb = 1.9 × 10-9  The dissociation equation of pyridine :…

Q: 5. To study the effects of a weakly acidic medium on a culture containing a new strain of bacteria,…

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Q: 2. How many moles of Ag Br can dissolve in 1.0 L of 0.40M NH;? Kr [Ag(NH3)2] *= 1.7 x 107 Ksp(AgBr)…

A: Given: Kf [Ag(NH3)2]+ = 1.7×107 Ksp(AgBr) = 5.0×10-13 We have to calculate the number of moles of…

Q: Calculate the molar concentration of cadmium(II) ion in equilibrium with solid Cd(OH)2 at pH =…

A: Solubility product constant (Ksp) of cadmium hydroxide (Cd(OH)2) solution is 2.5×10-14 The given…

Q: Which of the following statements is true about a 0.0100 molar sodium bicarbonate solution? The Ką…

A: Please find your solution below :

Q: An industrial chemist studying bleaching and sterilizing prepares several hypochlorite buffers.…

A: Given : a buffer solution with  1) concentration of weak acid i.e HClO = 0.200 M 2) concentration of…

Q: What is the pH of a solution composed of 0.40M HOBr and 0.40M NaOBr. Ka of HOBr is 2.6x10-⁹ 9.12…

A: Given concentration of [HOBr] = 0.40M [NaOBr] = 0.40M Ka of HOBr = 2.6 * 10-9

Q: Ethyl orange, an indicator, has a Ka of 2.0 x 10–4. The protonated form is red and the deprotonated…

A: Given : Ka = 2 x 10-4  thymol orange is an acidic indicator.

Q: A basic buffer is observed to have a pH of 8.79. Kb = 1.77 x 10–5 for ammonia at 25 oC. The…

A: pH of the solution is equal to the negative logarithm of hydronium ion. pH=-log(H3O+) Henderson…

Q: An analytical chemist is titrating 160.2 mL of a 0.3300M solution of nitrous acid (HNO,) with a…

A: Given: The reaction is as follows: HNO2(g) + KOH(l)   ⇌  KNO2(aq) + H2O.  The volume of HNO2, (V1) =…

Q: Calculate the concentration of free Zn2+ ion at equilibrium when 1.58x10-2 mol zinc sulfate is added…

A: Each zinc sulfate, ZnSO4 produces 1 Zn2+(aq) ion Hence moles of Zn2+(aq) ion added to 1.00 L…

Q: Cr2O72- + C2H5OH -> Cr3+ + CO2   How do you balance this equation in an acid solution?

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Q: could you please answer and show working to the following questions    1. What is the pH of a…

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Q: Which of the following is not best used as a titrant for the acid-base titration of antacid tablets?…

A: Answer: Antacid tablets are used in the remedy of acidity when pH of the stomach decreases and…

Q: a. NiO2 + 2 H2O + Fe→Ni (OH)2 + Fe(OH)2 in basic solution b. CO2 + 2 NH2OH→CO + N2 + 3 H20 in basic…

A: NiO2 + 2H2O →Ni(OH)2 + 2OH- Fe + 2OH- → Fe (OH) 2 On combining both the reactions, OH- will be…

Q: If you wish to use 20ml of 0.5M HCl to titrate [Ni(en)3]SO4, how many grams of [Ni(en)3]SO4 should…

A: The question is based on the concept of acid base titration. we have to calculate mass of complex…

Q: What is the pH value of the solution containing 0.085 M HNO2 and 0.1 M KNO2? (Ka: 4,5x10-4)

A: Given: Concentration of  HNO2= 0.085M Concentration of KNO2=0.1M Ka=4.5×10-4

Q: 28) Explain why the pH does not change significantly when a small amount of an acid or a base is…

A: A buffer solution is the solution which restrict the pH change on mixing small amount of an acid or…

Q: Given that the Kf for [Ni(H2O)5(NH3)]2+ is 501 and Ka for NH4+ is 2.0 x 10-5, what is the…

A: Given data, Ka for NH4+=2.0×10-5Kf for [Ni(H2O)5(NH3)]2+=501

Q: A sample of water (200 mL) was titrated by 0.05 M H2SO4. The titration completed when the color…

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Q: Ethyl orange, an indicator, has a Ka of 2.0 x 10–4. The protonated form is red and the deprotonated…

A: ethyl orange is a pH indicator frequently used in titration because of its clear and distinct color…

Q: A solution of 0.021 M AgNO₃ that is also 1.23 M NH₃. The kf for Ag(NH₃)₂⁺ is 1.7x10⁷. In a 1.5L of…

A: Given: Concentration of Ag+ (From AgNO3) = 0.021 M Concentration of NH3 = 1.23 M Volume of solution…

Q: 14. Calculate the concentration of Ag + in the solution of 0.10 M [Ag(NH3)2] (dissociation constant…

A: Given: Concentration of [Ag(NH3)2]+ = 0.10 M And dissociation constant for [Ag(NH3)2]+ = 6.3 × 10-8…

Q: 15. What is the molar solubility of Mg(OH)2 in an aqueous solution buffered at pH 12.2.(Solubility…

A: Answer: we have to calculate molar solubility of Mg(OH)2 if ksp is given Explanation:  Mg(OH)2 -&gt;…

Q: Which of the following contains a set of incorrectly paired words? * Chelatometry - Complexation /…

A: Here we have to choose the incorrectly paired words and Lewis base in a complexation reaction-

Q: Will the aqueous solutions be acidic, basic, or neutral? a. Ca(CN)2 b. Fe(NO3)3

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Q: 1.) Which of the following is the correct equilibrium constant for the following reaction? KCIO4 (s)…

A: Question 1. Equilibrium constant is the ratio of( product of) concentration of products  to the…

Q: 16.94. Fluoride and Dental Hygiene Fluoride ions in drinking bortita water and toothpaste convert…

A: Since in hydroxyapatite we have OH ions present which will have much more tendency to form H bonds…

Q: A 2.0 L solution contains 1.0 mol of sodium formate (NaCHO,). What is the pH of this solution after…

A: Henderson - Hasselbach equation is used to calculate the pH of buffer solution .  pH = pKa +…

Q: Given that the Kf for [Ni(H2O)5(NH3)]2+ is 501 and Ka for NH4+ is 2.0 x 10-5, what is the…

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Q: Which set of reagents can confirm that sulfate ions are present in two unkown solutions? a.1.0 M…

A: Solution: Test for sulfate ions Sulfate ions SO42-, are detected using barium chloride / barium…

Q: Which salts will be more soluble in an acidic solution than in pure water? Sn(OH)2 AgBr KClO4 CaCO3…

A: The fact to these is knowing what anions react with H^+ (the acid) and if any weak acids or…

Q: Rank the following salts in order of INCREASING pH of their 0.1 M aqueous solutions   1 2 3 4 KNO3…

A: pH is the measure of acidity or basicity of the solution. A solution with pH below 7 is acidic while…

Q: Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To…

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Q: 20. The pH of buffer solution containing 0.2 mole/ liter of CH;COOH & 0.2 mole/I of CH;COONA has…

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Q: What is the maximum [CO32-] that can exist in a solution of 7.1 x 10-7M AgBr?

A: [AgBr] = 7.1 x 10-7 M

Q: What concentration of SO 3 ^ 2- is in equilibrium with Ag2SO3(s) and 1.60 x 10^-3 M Ag^+?

A: [Ag+] = 1.60 x 10-3 M  Ksp of Ag2SO3 = 1.5×10-14

Q: Choose the buffer with the greatest buffering  capacity:     d. 0.25M formic acid/formate buffer at…

A: We are given three different types of buffer solution at different pH and concentrations and we have…

Q: Calculate the values of the buffer capacity at pH = 7 and pH = 9 in 0.08 M ammonium chloride…

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.