A 0.15 M solution of a weak acid is 3.0% dissociated. Calculate Ka.

Q: You can find the Ka of a strong acid by running a titration curve.

A: The use of dissociation constant is to measure how well an acid or a base is been dissociated. For…

Q: FeCl3

A: FeCl3 is a salt of strong acid HCl and weak base Fe(OH)3. When the salt forms the solution will be…

Q: A 10.0mL solution of aspirin (weak monoprotic acid) required 8.4mL  Of 0.0245M NaOH to reach…

A: Question is about the titration of a solution of Aspirin with NaOH solution. We have to calculate…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.431.43 M solution. The pH of the…

A:

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0137 M solution. The pH of the…

A: Since the acid is weak monoprotic acid. Hence we can assume it to be HA

Q: What is the pH when 100 ML of 1M NaOH is added to 200 mL of 2M acetic acid? pKa of acetic acid= 4.76…

A: Given,The molarity of CH3COOH = 2 MVolume of CH3COOH = 200 mLThe molarity of NaOH = 1 MVolume of…

Q: The K, of a monoprotic weak acid is 0.00728. What is the percent ionization of a 0.148 M solution of…

A: monoprotic acid: A monoprotic acid donates only one proton or hydrogen atom per molecule to an…

Q: A buffer solution is prepared by taking 0.438 moles of acetic acid (pKa=3.45) and 0.736 moles of…

A: We have to predict the pH of the solution.

Q: The Ka of a monoprotic weak acid is 0.00638. What is the percent ionization of a 0.127 M solution of…

A:

Q: What is the pH of a solution prepared by mixing 59.50 mL of 0.8820 M HCl and 35.67 mL of 0.7859 M…

A: First we need to calculate moles of both HCl and NaOH and then Calculate excess moles remaining…

Q: PR: (a) Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate…

A: Part (a): Initial pH Calculation For a buffer solution of cyanic acid (HCONO) and sodium cyanate…

Q: Calculate the pH of a 0.30 M solution of sodium benzoate. Benzoic acid has a K₂ of 6.46 x10-5. 8.83…

A: sodium benzoate is the salt of weak acid (benzoic acid) and strong base (NaOH). so Here salt…

Q: Write the chemical reactions whose equilibrium constants are K, and K, for imidazole (C, H, N,) and…

A:

Q: Calculate the pH of each solution that is buffered. (a) 0.100 L of 0.25 M NH4Cl + 0.050 L of 0.25 M…

A: In the above question Kb of NH3 is not given so the standard  value of Kb of NH3 is 1.8 x 10-5 which…

Q: Coleiro-ic Acid, HColeiro , is a new organic compound used to manufacture hypnotic drugs and some…

A:

Q: compound Cr(CIO4)3 KCN Nal solution is...? acidic basic O neutral acidic basic O neutral O acidic…

A: Hydrolysis of salt. Cation and anion part of the salt under go reaction with water to give…

Q: d) Why is the pH of mixture D the same as the pH of mixture B?

A: Answer: pH tells us about the strength of hydrogen ion concentration in the solution. Its value is…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.37 M solution. The pH of the…

A:

Q: a) If potassium nitrite (KNO₂) and sodium nitrite (NaNO₂) are dissolved in water, select the choice…

A: Answer: Strong acid gets completely ionized in its solution while weak acid gets partially ionized…

Q: Given the data for the following separate titrations, calculate the molarity of the NaOH: mL HCI…

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Q: Calculate the pH change that results when 11 mL of 5.1 M NaOH is added to 790. mL of each the…

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Q: Would a 1 M solution of just acetic acid resist increases to pH, decreases to pH, neither, or both?…

A: 1M acetic acid is acidic, because Ka value of acetic acid is greater than kb value of its conjugate…

Q: A weak monoprotic acid is 4.3% ionized in solution at equilibrium. Find the pH of the solution and…

A: The pH of a solution is the negative logarithmic of hydronium ion concentration in the solution.

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.18M solution. The pH of the…

A:

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0147 M solution. The pH of the…

A: Since the acid is a weak acid so it dissociates partially so the degree of dissociation is not high.

Q: Ascorbic acid C5H7O4CO2H (Ka =7.9x10^-5) also known as vitamin C is an essential nutrient for all…

A:

Q: A chemist titrates 60.0 mL of a 0.5980M hypochlorous acid (HCIO) solution with 0.6753M NAOH solution…

A: At equivalance point , both acid and base neutralize each other to give conjugate  salt  . So moles…

Q: The pOH of an aqueous solution of 0.532 M acetylsalicylic acid (aspirin), ( Ka (HC9H7O4) = 3.0 ×…

A:

Q: 2. A solution contains 250 mL of 0.25M benzoic acid (HBen) and 0.20M sodium benzoate (NaBen). What…

A: Step 1:Ka= 6.5×10-5pka= -(log Ka)      =-(6.5×10-5)      = 4.18 Step 2:HCl is strong acid when added…

Q: Part B. 1. The hydrogen ion concentration in a solution is measured to be 7.84 X 10-5 M. Calculate…

A: The pH is given by pH = -log10[H+]

Q: The pH of a 0.095 M solution of an unknown monoprotic acid is 5.42. Calculate the Ka of the acid.

A:

Q: 16.82 Brown) Using data from appendix D (or any online weak acid table), calculate [OH-] and pH for…

A: (1)  F-+H2O  ⇌ HF + OH-concentration F- = 0.105 MKa = 6.8×10-4Kb = KwKa = 10-146.8×10-4 =…

Q: Calculate the pH of the following: 5) A solution that contains 0.10 M ammonium hydrochloride and…

A: In this solution we have a strong acid HCl which dissociate completely .  And another is a weak acid…

Q: explain why the ph doesnt change significantly when a small amount of an acid or a base is added to…

A: pH doesn't change significantly when a small amount of an acid or a base is added to a solution that…

Q: 2. Calculate the pH of a solution made by mixing 100.0 mL of 0.110 M NaBrO with 75.0 mL of 0.140 M…

A: Given:Initial concentration of NaBrO, M1 (NaBrO)= 0.110 MInitial volume of NaBrO, V1 (NaBrO)= 100.0…

Q: A solution which is yellow in the presence of alizarin yellow indicator and red in the presence of…

A: Based on the precision of the indicators shown in the picture, alizarin yellow has a pH range of…

Q: A 20.0-mL sample of 0.200 M HBr solution is titrated with0.200 M NaOH solution. Calculate the pH of…

A: HBr  + NaOH  ------->  NaBr   + H2O millimoles of HBr = M x V = 0.2 x 20 = 4 mmol millimoles of…

Q: An analytical chemist is titrating 139.2 mL of a 0.2600M solution of ammonia (NH3) with a 0.5900M…

A: we have to calculate the pH of the solution

Q: A 0.150 M solution of a weak acid has a pH of 2.75. What is the Ka value of this acid?

A: Given that, The concentration of a weak acid is C = 0.150 M. The pH of that 0.150 M solution of warm…

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.