Calculate the pH of a 0.858 M0.858 M solution of sodium acetate (CH3COONa)?  Ka= 1.8x10^-5

Q: Q2// 1000 ml of o.1M hydrochloric acid were added to 1000 ml of o.1M ammonium hydroxide, ammonium…

A: Given that 1000 ml of 0.1 M hydrochloric acid and 1000 ml of 0.1 M ammonium hydroxide is reacted…

Q: A 0.17 M solution of a weak acid has a pH of 2.85. What is the ka of the weak acid?

A: Given: concentration of weak acid=0.17M              pH of weak acid=2.85 To calculate: Ka of weak…

Q: What is the pH of a 0.0640 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

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Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0176 M solution. The pH of the…

A: Given, Concentration of weak acid (C) = 0.0176 M pH of solution = 2.47 Dissociation constant (Ka) =…

Q: 3..A 10 mL solution of 0.38 M HA (pKa = 4.40) is mixed with 8.0 mL of 0.38 M KOH. What is the pH of…

A: Given-> Volume of HA = 10 ml Molarity of HA = 0.38 M Volume of KOH = 8.0 ml Molarity of KOH =…

Q: Calculate the pH of 50.0 ml of 0.250 M oxalic acid (HOOCCOOH) upon addition of 15 mL of 0.500 M…

A: Oxalic acid is a diprotic weak acid, whereas monoacidic NaOH is a strong base. Given the volume of…

Q: What is the pH of a solution that is 0.12 M in HOCl and 0.20 M in NaOCl?  Ka of HOCl is 3.5 x 10-8…

A: Given, 0.12 M in HOCl and 0.20 M in NaOCl

Q: Calculate the pH of a solution when 10.00 mL of 0.1000 M NaOH is added to 20.00 mL of 0.1000 M…

A: Given: Concentration of CH3COOH = 0.100 M Volume of CH3COOH solution = 20.00 mL = 0.020 L…

Q: Calculate the pH of a solution containing 0.0361 M benzoic acid (HC>H502) and 0.0263 M sodium…

A: The given mixture is a buffer solution mixture. So, this can be solved from the Henderson…

Q: What is the pH of a solution that is 0.20 M potassium cyanate, KCNO and 0.16 cyanic acid HCNO? The…

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Q: The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization…

A: Given : We have to calculate the ionization constant.

Q: What is the pH of a solution which is 0.023 M in weak base and 0.035 M in the conjugate weak acid…

A: The solution is as follows:

Q: What is the pH of a solution that is 0.21 M CH3NH2 (methylamine) and 0.31 M CH3NH3Cl (methylammonium…

A: Since CH3NH2 is a weak base with pKb = 3.38 And the solution is having CH3NH2 and its conjugate acid…

Q: What is the pH of a solution that is 0.33 M KOCN and 0.10 M HOCN (cyanic acid)?

A: pH is mathematically defined as negative logarithm of hydronium ion. pH=-log(H+).…

Q: Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M…

A: HC3H5O2 is a weak acid and dissociates in aqueous solution as: HC3H5O2+H2O↔C3H5O2-+H3O+

Q: Propanoic acid (CH3CH2COOH) is a moderately weak acid, with Ka = 1.3 x 103 at 25.0 °C. Calculate the…

A: Acidic Buffer :-  A mixture of weak acid and its conjugate base is called as acidic buffer solution…

Q: What is the pH of a solution containing a mixture of 0.050 M HC2H3O2 and 0.025 M NaC2H3O2?  (Ka =…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: The pH of 750 mL (3 SF) of an aqueous solution containing only NaNO 2 is 8.42. If HNO 2 has a Ka of…

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Q: What is the pH of an aqueous solution with .5 M NH3 & .45 M NH4Cl?  Kb=1.78 x 10-5

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Q: What is the pH of a 0.710 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

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Q: What will be the pH of 0.025 M NaOH solution in H2O at 60 °C? (KW60°C = 1.0 x 10-11) A. 1.6 B. 9.4…

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Q: find the pH of a 0.20M solution of a weak acid (ka =0.0332). 1.18 0.70 1.09 0.20

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Q: Calculate is the pH of 0.02 M HC2H3O2? Ka= 1.8x10^-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: What is the ph of a 0.10M solution of NaOCL(aq) For HOCl, Ka= 2.8x10^-8

A: Given, The concertation of HOCl is 0.1 M Ka = 2.8 x 10-8 Formula Used, pH = -log [H+]

Q: The pH of dissolving 1.48g of propanoic acid in 200ml of H2O is ---- If Ka=1.3*10^-5

A: Given that -  Mass of propanoic acid = 1.48 g  Volume of Solvent, H2O  = 200 mL  Acid Dissociation…

Q: What is the pH of a solution containing 0.1279 M HOCN and 0.1517 M KOCN? Ka = 3.50e-4.  10.544…

A: Acid, [HOCN] = 0.1279 M Salt, [KOCN] = 0.1517 M Ka = 3.50 × 10-4

Q: Butyric acid, C3H,COOH, has ionization constant of 1.54 x 10-5. a) Calculate the pH of 50.0 mL of a…

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Q: Calculate the pH of 100.00mL of 0.15 M HF solution after 131.00 mL of KOH 0.15 M have been added. Ka…

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Q: pH calculation at the initial point: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH)…

A:

Q: used as preservatives in vinegar, soy sauce, etc. The pH of a 0.10 M aqueous solution of sodium…

A: Sodium benzoate is salt of weak acid-strong base type salt pH = 1/2(14 + pKa + log([C]) 8.60 =…

Q: Calculate the pH value of 0.00 * ? acid at 25 C if Ka=0.0O00018 3.1

A: Given:  0.001M acetic acid at 25C if Ka = 0.000018   To find: pH value of 0.001M acetic acid at 25C…

Q: You have a 48.5 g mixture that contains potassium propanoate (CH3CH2COOK) and Propanoic acid…

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Q: The pyridinium ion (C5H4NH*) is a weak acid (Ka = 5.60 x 10-6). Calculate the pH of a solution that…

A: Given that, the pyridinium ion is a weak acid. The Ka of it is Ka = 5.60×10-6. 3.7 mL of 0.167 M of…

Q: What is the pH of a solution of 0.35 M Hydrochloric Acid?   60 35 68 7 45 61 75 90 80

A: HCl -------> H+ + Cl- [HCl] =0.35 M pH = -log [H+]

Q: An unknown weak acid with a concentration of 0.085 M has a pH of 1.80. What is the Ka of the weak…

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Q: What is the pH of a solution that is 0.26 M CH3NH2 (methylamine) and 0.38 M CH3NH3Cl (methylammonium…

A: The basic buffer may be explained as the solution mixture which hold the weak base along with its…

Q: 70 ml of an aqueous solution of 0.085 M acetic acid. It has a Ka=2.25x10^-4. Calculate the ph of the…

A: In the presence of strong acid the dissociation of weak acid is suppressed due to common ion effect…

Q: What is the pH of a solution with 10.2mL 0.10M CH3COOH and 0.15mL 1.0M HCl ? Ka = 1.8x10^-5

A: pH is the negative logarithm of the hydrogen ion concentration. It is a measure of acidity or…

Q: When answering this problem, report the answer with the appropriate number of significant figures…

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Q: the pH of a solution of 15 g NH4Cl and 15 g of NH3 in a 850mL solution? The Kb for NH3 is 1.8 x 10-5

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Q: Calculate the pH of a solution that is 0.20 M HOCI and 0.88 M KOci. Kg = 3.5x10-8 pH =

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Q: If the Ka of a monoprotic weak acid is 1.4×10−6, what is the pH of a 0.14 M solution of this acid?

A: Given information: Concentration of an acid = 0.14 M Ka of weak acid = 1.4×10-6

Q: a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: HIO3 has a ka of  0.16. What is the pH of a 0.600 M HIO3 solution? (use successive approximations)

A: The strength of an acid depends on the extent of its dissociation in water. Strong acids dissociate…

Q: Find the pH of a 0.4M aqueous hydrocyanic acid solution. For HCN, Ka=4.9 x 10^-10     4.85…

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Q: Calculate the pH of a 0.20 M C2H5NH2 solution. Kb=5.6x10-4

A: C2H5NH2 is a weak base. pH of this solution  = 12.04

Q: What is the pH of a solution prepared by adding 66.0 ml of 0.100 M HNO3 to 72.2 mL of 0.31 M NaOH?

A:

Q: Calculate the pH of a solution made by mixing 50.00 mL of 0.100 M NaCN with (a) 4.20 mL of 0.438 M…

A: You have posted 2 different  questions simultaneously, so I have to solve the first one that is 5…

Q: What will be the pH of a solution of a weak acid (HB), of concentration 0.15 M (Ka = 1.8x10-5

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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.