A certain organic amine acts as a mono acid base in an aqueous solution. A 0.05M solution has a hydroxyl ion concentration of 7.5x10 ^ -3. What is the pH value of the solution? What is the constant of the base? What is the value of the pkb?

Q: pH

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Q: A.) In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of…

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Q: A 1.0 M solution of a compound with 2 ionizable groups (pKa’s = 6.2 and 9.5; 100 mL total) has a pH…

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A: pH of a 0.428 M aqueous solution of trimethylamine, (CH3)3N to be 11.731 Kb for this experiment is…

Q: An analytical chemist is titrating  178.6mL  of a  0.3700M  solution of methylamine  CH3NH2  with…

A: The balanced reaction is as follows: CH3NH2+HIO3→CH3NH3++IO3- Calculation of no. of mol of CH3NH2:…

Q: The simplest amino acid is glycine ( molar mass = 75.1 g/mol), whose structure is shown above. An…

A: molarity = ωGmω × 1000V(mL)Given weight of glycine = 0.329 g                                V = 150…

Q: Calculate the pH, [H2L*], [HL], [L] for each solution of the amino acid proline (Kal = 1.12 x 102…

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Q: Determine the pH of a solution that is prepared by dissolving 1.9 g of Ba(OH)2 in 3.8 L water at…

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Q: Calculate the pH of a 0.020 M solution of phenylacetic acid, C6H5CH2COOH. What will be the pH if the…

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Q: Solution of glucose (concentration 1g/L) is diluted 1 : 10 and then 1 : 5. What is its  final…

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Q: Diethylamine, (CH3CH2)2NH, has a Kb of 8.6 x 10-4.  What is the pH of a 0.22 M solution of…

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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: Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer…

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A: Given:

Q: 2. Do you expect the equivalence point to be below a pH of 7, equal to a pH of 7, or above a pH of…

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Q: 1.0m HCl solution has a volume of 60.0mL. Calculate pH of the solution that results from 3.00g of…

A: Calculate the total number of moles of HCl and sodium acetate. The number of moles of HCl is…

Q: Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer…

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Q: How many milliliters of 2.5M benzoic acid need to be added to 500. mL of a solution already contains…

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Q: Determine the pH of a solution that is prepared by dissolving 8.7 g of Ba(OH)2 in 2 L water at 25°C.…

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Q: What is the pH of the solution that is prepared by dissolving 0.844 g of lactic acid (90.08 g/mol,…

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Q: needs from the soil if its pH is above 6.5. (a) The hydrogen ion concentration of a soil sample is…

A: A) [H+] =1.58×10-7 pH = -log([H+])  = -log(1.58×10-7) = 6.8 So, pH = 6.8

Q: What is the pH of a 0.010 M solution of acetic acid? Ka for acetic acid is 1.8x10^-5

A: The acid that dissociates partially in an aqueous solution is termed as the weak acid. Example;…

Q: Calculate the pH and the equilibrium concentrations of HC6H6O6- and C6H6O62- in a 0.2410 M ascorbic…

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Q: Find the pH of a 0.100 M ascorbic acid (H2C6H6O6) solution.

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Q: The pH factor is a measure of the acidity and alkalinity of water. A reading of 7.0 is neutral;…

A: Given data: 7.3, 7.4, 7.2, 7.0, 7.5, 7.4, 7.3, 7.3, 7.2, 7.1 n = 10 α = 0.05

Q: Determine the pH of a 0.62 mol L-1 NH4NO3 solution at 25oC. The Kb for NH3 is 1.76 x 10-5. Select…

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Q: An analytical chemist is titrating 110.0mL of a 0.5600M solution of butanoic acid HC3H7CO2 with a…

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Q: Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer…

A: Given: Concentration of salt= 0.52 M pH of buffer solution = 10.1 Kb of ethylamine = 5.6×10-4

Q: Calculate the pH when 1.03 g of NaClO (FW = 74.44 g/mol) is added to 44.4 mL of 0.50 M HClO. Ignore…

A: Answer: In this question we have to calculate the pH of the buffer made of HClO and NaClO.

Q: The Henderson-Hasselbalch equation for the reaction can be written as :  pH = pKa + log ([A–]/[HA])…

A: The Henderson-Hasselbalch equation for the reaction can be written as :  pH = pKa +log[salt][acid]…

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Q: 2. Write the dissociation equation and equilibrium constant expression for the dissociation of the…

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Q: Sodium formate (NaCHO2) is used in fabric dyeing and painting process.  Formic acid is the conjugate…

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Q: Methyl Amine (CH3NH2) is a weak base with a Kb of 4.38 x 10-4. What would be the pH of a solution of…

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Q: FOR THESE 4 GIVE ANSWER TO 2 DECIMAL PLACE IN REGULAR NOTAION: 1) Determine the pH of a 0.275 M KOH…

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Q: 0.369 mol of a weak base (pKb = 5.52) is added to 0.298 mol of the salt containing its conjugate…

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Q: 1. Calculate what pH should be for Mg2+ at 1.31 x 10-2 concentration. (Mg(OH)2(s) Mg2+ (aq) +…

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Q: A.) In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of…

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Q: Given,  Molarity of glycine hydrochloride (say HA) = 0.1 M  Volume of glycine hydrochloride = 20…

A:

Q: An acid mixture contains 0.60 M HClO (Ka = 2.9 × 10−8) and 0.50 M H2O2 (Ka = 2.4 × 10−12).  What is…

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Q: Consider the following solutions: Solution 1: 0.100 L of 0.25 M NaCH3CO2 + 0.050 L of 0.25 M HCl…

A: # Solution-1: Volume of 0.25 M  NaCH3CO2 = 0.100 L Moles of NaCH3CO2  = C*V= 0.25 molL * 0.100 L=…

Q: An analytical chemist is titrating 149.0mL of a 0.2200M solution of piperidine C5H10NH with a…

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Q: CH3NH2 is a weak base (Kb=5.0×10−4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a…

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Q: Calculate the pH of the following mixture 500 ml 0.35 M CH3CH2NH2 + 500 ml 0.25 M HNO3

A: Given : The volume of CH3CH2NH2= 500 ml Molarity of CH3CH2NH2 =0.35 M The volume of HNO3=500 ml…

Q: the solution of 2.50 L of a 0.250M CH3CO2H has a pH of 4.20, what is the pH if you add 20.0 mL of…

A: At equilibrium,                              CH3COOH  ⇌  CH3COO-  +  H+  The pH of this solution can…

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.