Why is H3O=[OH- ]=1.0 x 10-2 M not feasible in water? What would happen if we tried to make such a solution by mixing 1.0 x 10-2 molL of KOH with 1.0 x 10-2 molL HCl?

Q: What is the pH of a 5.0×10-2 M solution of KOH at 25 °C?

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Q: What are the concentrations of OH− and H+ in a 0.00069 M solution of Ba(OH)2 at 25 °C? Assume…

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Q: What is the percent ionization of H2NNH2 in a solution with a concentration of a 0.560 M? (Kb = 1.3…

A: Given information,  H2NNH2 in a solution with a concentration of a 0.560 M  Kb = 1.3 x 10-6

Q: What is the [H3O] in a solution 1.50x10-4M Ca(OH)2?

A: Ca(OH)2 -----> Ca+2 + 2OH- [Ca(OH)2] = 1.50x10-4 M

Q: 11. What volume of 0.115 M HCl solution is needed to prepare 350.0 mL of a solution of HCl with pH…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: Calculate the pH of a 5.3 x 10-3-M solution of H2S04 (Ka, = 1.2 x 10-2). pH =

A: Given-> Concentration of H2SO4 = 5.3 × 10-3 M

Q: A diprotic acid (H₂A) has Kai - 4.55 x 10-7 and K₁2 = 6.07 × 10-¹¹. What is the pH of a 0.463 M H₂A…

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Q: What concentration of NaF is required to make [H3O+] = 2.3 × 10−4 in a 0.300-M solution of HF?

A: HF is a weak acid and NaF is the salt of its conjugate base. Thus , the given solution is buffer…

Q: At 25 degrees Celsius, what is the hydronium ion concentration in 0.100 M sodium chloroacetate? O a.…

A: Given,  Concentration of Sodium chloroacetate, ClCH2OONa is = 0.100 M

Q: Determine the pH of a 0.22M NaF solution at 25 degrees Celsius. The Ka of HF is 3.5 x 10-5

A: We have to calculate the pH of 0.22 M NaF solution.

Q: An aqueous solution at 25 °C has a OH concentration of 1. x 10 ´M. Calculate the H,O' concentra x10

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Q: What is the pH of a solution at 25°C in which [NaOH] = 3.14 x 10-5 M

A: Given :-  [NaOH] = 3.14 × 10-5 M  To calculate :-  pH of solution

Q: Determine the OH-, pH, and pOH of a solution with a H+ of 4.5 x 10-6 M at 25 °C. [OH"] = pH = pOH =

A: Solution pH and pOH defined as the   negative log of concentrations of hydrogen or hydronium ions.…

Q: Calculate the OH- for a 0.300 M solution of pyridine, Kb = 1.7 x 10^-9

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Q: What are the concentrations of  OH−  and  H+  in a  0.00080 M  solution of  Ba(OH)2  at  25 °C?…

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Q: What is the pH and the pOH of a 0.0215 M HCIO3 solution at 80.0 °C? Kw 2.5 x 10-13 at 80.0 °C pH:…

A: Given: Kw=2.5×10-13 [HClO3]=0.0215 M To find: pH and pOH Formula: pH=-log10[H+] pH+pOH=14

Q: What is the pH of a solution with [OH1-] = 1 x 10-8 ?

A: Since, pH represent the acidity of the solution. If pH less than 7 then solution is acidic. If pH =7…

Q: iv) What name is given to the solution formed when all the NaOH has reacted? Calculate the p" of the…

A: The question is based on the concept of titrations. we are adding acetic Acid to the sodium…

Q: What is the pOH of an aqueous solution of 4.90×10-2 M potassium hydroxide? pOH = ______

A: KOH is Strong base so it's pOh can be easily Calculated by Poh= -log[OH-] POH is the power of OH-…

Q: 2. What is the pH of 0.0072 M NaOH? 3. What is the pH of 0.00343 M Ba(OH)2? 4. If pOH of a solution…

A: Hi, we are supposed to answer one question. To get the remaining questions solved please mention the…

Q: Why is [H3O]=[OH]=1.0*10-2 M not feasible in water? What would happen if we tried to make such a…

A: Since the water has an equilibrium with H3O+ and OH- ions as per the reaction  2 H2O (l)…

Q: Calculate the pH of 0.02354 M CH3 CO2 H and 0.1702 M NaCH3 C02. {Ka = 1.8 x10 °}

A: Given: [CH3CO2H]=0.02354 M [NaCH3CO2]=0.1702 M pH=? Ka=1.8 x 10-5

Q: Hydroxylamine (NH2)H) is a weak base with a Kb=6.6x10^-9.  What is the pH of a 0.36 M solution of…

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Q: What is the OH- ion concentration of 8.8 x 10-4M Sr(OH)2 solution?

A: Given;

Q: In an aqueous solution at 25 C, if [H3O+]=3.1×10^-4M, then [OH-] is

A: Given data: The hydronium ion concentration is H3O+=3.1×10-4 M. To find: The hydroxide ion…

Q: pH

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Q: When [H+]=4.0 x 10(-9) M in water at 25 C, what is the pH

A: Given that Concentration of H+ = 4.0×10-9 M

Q: What is the pH of a 0.85 M H2SO4?   Show your ICE table and calculations.  Ka1 for H2SO4 is a very…

A: The sulfuric acid completely disassociates in the solution, hence we can assert that the…

Q: What is the pH of a 3.9×10-2 M solution of KOH at 25 °C?

A: KOH ionizes in aqueous solution as,                          KOH (aq)       -----> K+ (aq)   +…

Q: For a 1.0 x 10-6 M solution of HNO3(aq) at 25 °C, arrange the species by their relative molar…

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Q: 16. At 50°C, the Kw is 5.47 x 10-14. At this temperature, pure water A. is neutral. B. is slightly…

A: Hydroxide and hydroxyl ion are equal in amount    hence PH and POH are same hence solution is…

Q: Which of the following statements is TRUE for a solution containing 0.01 M HF(Ka = 6.6 x 10^-4) and…

A: To find: Which among the following statements are true regarding 0.01 M HF(Ka = 6.6 x 10-4) and 0.01…

Q: What is the percent ionization of H¿NNH2 in a solution with a concentration of a 0.530 M? (Kb = 1.3…

A: Weak base dissociate partially in solution. The degree of ionization is not complete in such…

Q: Calculate the pH of an aqueous solution at 25°C that is (a) 0.035 M in HI, (b) 1.2 × 10-4 M in HNO3…

A: pH can be calculated by using the formula, pH=-log(H+)

Q: What is the pOH of a solution that contains 8 x 10-5 M HCI at 25°C?

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Q: The active ingredient formed by aspirin in the body is salicylic acid, C H OH(CO₂H). The carboxyl…

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Q: What is the pH of (3.21x10^-1) M C5H5NHBr?

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: 2. What is [OH ] in an aqueous system if the concentration of H*/H3O* is 5.0 x 10-5Ma

A: A numerical problem based on concentration of OH-, which is to be accomplished

Q: Based on the Kb determined in the previous part, what is the pH of the initial 1.0 M base solution?…

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Q: What is the pH of a solution with H30+ =4.5 × 10^-5  M? 5.4 6.2 11.0 4.3

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Q: An equation representing the reaction of a weak acid with water is O HCI + H20 H;O* + CF NH3 + H20 2…

A: The equation representing the reaction of weak acid with water is as follows ;

Q: -8 An aqueous solution at 25 °C has a OH concentration of 1.7x 10 °M. Calculate the H,0' concentrati…

A: [OH-] = 1.7 × 10-8 M Temperature = 25 °C [H3O+] =?

Q: Determine the [OH-], pH, and pOH of a solution with a [H+] of 3.4 x 10-5 M at 25 °C. [OH-] pH = POH…

A: Since, Negative logarithm of concentration of H+ ion is known as pH. Then,

Q: What value of 0.25 M HNO3 is necessary to fully neutralize 7.4 g of Ca(OH)2 when dissolved in water?

A: The ratio of number of moles of solute to the volume of solution in liters is known as molarity.

Q: What is the pH for a solution at 25 °C that has a OH" concentration of 3.08 ×10-4 M?

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Q: Determine the [OH-], pH, and pOH of a solution with a [H*] of 3.3 x 10-7 M at 25 °C. [OH¯] = M pH…

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Q: Calculate the pH of an aqueous solution at 25°C that is (a) 0.081 M in HI, (b) 8.2 × 10-6 M in HNO3…

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Q: What is [Al(H2O)5(OH)2+] in a 0.15-M solution of Al(NO3)3 that contains enough of the strong acid…

A: Al(NO3)3 give Al3+ (aq) ions Now Al3+ ions combine with H2O to form complex [Al(H2O)6]3+ We have…

Q: What is the pH of a 0.89x10-2 M solution of Ba(OH)2 at 25°C?

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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.