What is the equilibrium pH of an initially 0.37 M solution of a weak acid HA at 25°C? Ka = 4.89 x 10 for the weak acid. Please keep your answer to two decimal places.

Q: A weak acid, HA, has a p?apKa of 4.5424.542. If a solution of this acid has a pH of 4.4944.494, what…

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Q: weak monoprotic acid (HA) has an acid ionization constant Ka = 1.8x10° at 298 K. If 100 mL of a 0.10…

A: First write equilibrium equation for reaction of weak acid and strong base and fine limiting…

Q: An acid (HA) dissociates as follows: HA – H* + A minus Arrow should be interpreted as an equilibrium…

A: The equilibrium reaction given is, => HA --------> H+ + A-  Given : Initial concentration of…

Q: The weak acid, HA, has a Ka of 1.60 x 10-10. What is the Kb of its conjugate base, A™?

A: Given :-  Ka for weak acid (HA) = 1.60 × 10-10  To determine :  Kb of its conjugate base (A-)

Q: Enter your answer in the provided box. Determine the K, of a weak base if a 0.29 M solution of the…

A: The pOH of 0.29 M solution is calculated below.

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: Butyric acid  ( C3H7COOH) is a weak acid . What is the pH of a 0.0250 M solution of this acid. Ka =…

A: For weak acids, ions dissociation is very small that results in small H+ ions amount. Their…

Q: Do you think the pH of 1.0 M tri-methyl ammonium (CH3)3NH", pKa 9.80, will be higher or lower than…

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Q: Phenol is a weak acid with a Ka = 1.28 x 10-10. As a pure compound, it is rather corrosive but in…

A: The reaction taking place will be  PhOH ----> PhO- + H+ Assuming a concentration of PhOH is…

Q: 1. For each neutralization, state if the pH will be acidic (pH 7) when equal number of moles of…

A: According to the company guidelines, we have to answer only the first question. So, please kindly…

Q: The weak base methylamine, CH3NH2, has Kb= 4.2 x 10-4 . It reacts with water according to the…

A: Given: Kb= 4.2 x 10-4 Equation reaction: CH3NH2(aq) + H2O(ℓ) ⇌ CH3NH3+(aq) + OH-(aq) Concentration…

Q: Calculate the pH of a solution that is 0.0510 M in а. Н3РОД (Ка1 — 7.1 х 10 3). pH = b. НзРОз (Кal =…

A: It's a multiple part question.   Given information, Concentration of the given compounds = 0.0510 M…

Q: If 0.10 M aqueous solutions are prepared of each of the following acids, which produces the solution…

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Q: A weak acid HA has a Ka of 5.3x10-5. A solution of HA has a pH of 3.00 a) Calculate the initial…

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Q: A solution is prepared in which the concentration of propionic acid, HC3H5O2, is 0.250 M and the…

A: The given buffer solution is a mixture of weak acid propionic acid (C2H5COOH) and its conjugate base…

Q: ________ is found in carbonated beverages due to the reaction of carbon dioxide with water. Write…

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Q: For a given acid, Ka is 7.2  x 10−4. This means that it is: a strong acid B a weak base C a weak…

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Q: 3. Normal rainwater has a pH near 6. In rainwater that falls close to a coal-burning power plant,…

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

Q: What is the pH of a solution that is 0.15 M NH4Cl and 0.35 M NH3?   The Ka of NH4Cl is 5.01 x…

A: In this question , we have to calculate the correct pH of given problem by the help of…

Q: HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M…

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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: What is the pH of a 0.144 M solution of ammonia (Kb 1.8 x 10-5)?

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Q: If you mix 100. mL of 0.11 M HCl with 50.0 mL of 0.22 M NH3, what is the pH of the resulting…

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Q: Determine the pH of a solution of a weak acid (HA) that is 0.17 M. The Ka of the weak acid is 7.5 x…

A: Given a concentration of weak acid (HA) =0.17M Acid dissociation constant value =        7.5 x 10-5…

Q: a value of 7.2 x 10*. What is the pH to 2 decimal -f hydrofluoric acid with a concentration of 0.537…

A: We will calculate pH

Q: Aniline, C6H5NH2, is a weak base with K, = 3.8 x 10-10. What is the pH of 0.750 M anilinium chloride…

A: Anilinium chloride is a salt made from strong acid HCl and weak base aniline.  So, solution of…

Q: Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places.…

A: PH  of solution determines the nature of solution whether it is acid or basic solution. The acidic…

Q: A hypothetical weak base has Kb = 5.0 × 10−8. Calculate the equilibrium concentrations of the base,…

A: Given: Kb for the weak base = 5.0 × 10-8  Concentration of the weak base = 0.15 M We have to…

Q: H* = 1,0X 10"" -12 PH> ? OH = ? Acidic or Basic 2

A: Given information,         The concentration of hydrogen ion is 1.0 * 10-12 M

Q: The substance benzoic acid (C6H5COOH) is a weak acid (Ka = 6.3×10-5).What is the pH of a 0.258 M…

A: 1) Given: Concentration of C6H5COOK = 0.258 M The hydrolysis reaction of C6H5COO- coming from…

Q: If 0.10 M aqueous solutions are prepared of each of the following acids, which produces the solution…

A: The concentration of all the acids given are same. Also, all the given acids are monoprotic acids.…

Q: What is the pH of a 3.0 x 10 M solution of CoHsNH2 (Kb= 4.3 x 1010? What is the percent error in…

A: As PhNH2 is an weak base,it can be calculated using a formula.

Q: If the Ka of a monoprotic weak acid is 6.6x10-6, what is the pH of a 0.32 M solution of this acid?

A: Ka = 6.6 x 10-6 c = 0.32 M

Q: The Ka for cyanic acid HOCN is 3.5 x 10-4. What is the pH of a 0.37 M solution of the acid? What is…

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Q: The acid dissociation constant K of boric acid (HBO3) is 5.8 × 10¯¹0. Calculate the pH of a 2.5 M…

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Q: Calculate the [OH-], [H3O+], pOH and pH of a 0.075 M NH3 Ka NH4+ = 5.70 x 10-10

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Q: Calculate the pH of a 0.561 M solution of a triprotic weak acid, H3A, given the acid ionization…

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Q: Consider 1M solutions of each of the following acids (with their Ka values). Which solution would…

A: The question is based on the concept of acidity. we have to identify which of the given acid has…

Q: For propanoic acid (HC3H5O2, K, = 1.3 x 10), determine the concentration of all species present, the…

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Q: Determine the pH of a solution of a weak acid (HA) that is 0.0072 M. The Ka of the weak acid is 1.9…

A: Given ,  Weak acid is HA Concentration of weak acid (C) = 0.0072 M Dissociation constant (Ka) of the…

Q: What is the pH of a 0.15 M solution of the weak base, ammonia, NH3 (Kb = 1.8 x 10-5) in water? (SHOW…

A: Ammonia is a weak base, when it reacts with water it forms hydroxide ion. aAt equilibrium the…

Q: Enter your answer in the provided box. What is the pH of a 0.116 M monoprotic acid whose K, is 5.275…

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Q: A particular sample of vinegar has a pH of 2.90. If acetic acidis the only acid that vinegar…

A: The acetic acid formula is CH3COOH found in vinegar pH =-log[H+] The dissociation constant (Ka) =…

Q: A diprotic acid, H2A, has Ka1 = 3.4 x 10 4 and Ka2 = 6.7 x 10-9. What is the pH of a 0.28 M solution…

A: Given: The molarity of the solution of H2A is 0.28 M The value of Ka1 is 3.4 x 10-4 The value of Ka2…

Q: The Ka for HC2H3O2 is 1.8 x 10-5. What is the pH of a 0.02M solution of this weak acid?

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Q: Calculate the pH of a 0.10M weak acid, HA, whose Ka is 1.8 X 10

A: Given that: Concentration of weak acid,(HA) = 0.10M Ka = 1.8×10-5 Weak acid partially dissociates…

Q: The formula for the pH of a solution of hydronium ions is given by the logarithmic equation pH = -…

A: We will calculate the pH by using its formula.

Q: For the diprotic weak acid H₂A, Kal = 2.8 x 10-6 M and K₁2 = 8.9 x 109 M. What is the pH of a 0.0450…

A: Introduction :  Diprotic acid are those acids which produces two moles of hydrogen when they are…

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.