What is the pH of a 0.380 M solution of ethylamine? 8.5 1.9 10.2 5.5 12.1

Q: If a urine sample has a pH of 5.50, calculate the concentrations of H3O+ and OH− in the sample.

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Q: A 5.0M solution of acetic acid (pKa=4.75) has a pH of 6.75. The ratio of acid to conjugate base is?

A: The pH of a buffer is calculated by Henderson-Hasselbach equation. pH=pKa+log[conjugate…

Q: A sample of a cleaning product containing household ammonia, has a pH of 10.5. Determine the…

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Q: The Kb of dimethylamine [(CH3)2NH] is 5.90×10-4 at 25°C. Calculate the pH of a 1.15×10-3 M  solution…

A: [H+] [OH-]  =  10-14 PH + POH  = 14 [OH-]  = 10-14/ [H+] [H+]  =  10-14               [ OH-]

Q: Calculate the hydronium ion concentration in an aqueous solution that has a pH of 6.65

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Q: Calculate the [OH−] and the pH of a solution with an [H+]=6.3×10−10 M at 25 °C. [OH−]=     M pH=…

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Q: Calculate the hydroxide ion concentration of a solution with a pH of 12.65. O 0.022M 0.18M 0.56M…

A: PH is defined as power of hydrogen, it is negative logarithm of H+ ion concentration.

Q: Calculate the pH for an aqueous solution of pyridine that contains 4.15 x 10^-4 hydroxide ion. Group…

A: Given, [OH-] = 4.15×10-4 M pOH = -log[OH-] pOH = -log[4.15×10-4 ] pOH = 3.38

Q: The Kb of methylamine is 4.4 x10-4.  What is the pH of a 0.35 M solution of methylamine? 11.56…

A: Arrhenius theory of electrolytic dissociation assumes that a dynamic equilibrium exist between ions…

Q: 42) What is the [H3O+] concentration of a solution that has a pH = 11.61, 7.156, 0.015

A: pH = -log [H+] = - log [H3O+] pH = - log [H3O+] [H3O+] = 10-pH   Use this formula to solve for…

Q: (3 points) The pH of a sample of soap solution is 10.80. Calculate its molar hydronium…

A: 4th option is correct. Solution is given in step no 2:

Q: Calculate the H3O+ concentration in a sample of acid rain with a pH of 3.90.

A: pH is defined as the negative logarithm to the base 10 of hydronium ion concentration expressed in…

Q: Calculate the pH of a 0.307 M NH3 solution. NH3 has a ?b=1.8×10−5.

A: First of all a balanced reaction should be written for the solution: Here, water concentration is…

Q: A sample of a cleaning product containing household ammonia, has a pH of 11.5. Determine the…

A: Given  PH     = 11.5  [OH-] =  ?

Q: 36. Determine the pH of 0.25 M HBr solution.* A. 0.30 O B. 0.52 C. 0.60 O D. 13.0

A: 1 mol of HBr contains one mole of each H+ and Br- ions each.

Q: What is the pH of 0.15 M solution of acetic acid (CH3COOH) Ka=1.75 x 10^-5 A) 2.6 x 10^-6 B) 0.0016…

A: Calculating pH of the acetic acid. CH3COOH + H2O <----------> CH3COO- + H3O+

Q: A substance that is very acidic may have a pH of 1 or 2. This means that the acidic substance: Group…

A: We know, pH is the negative logarithm of the hydrogen ion concentration of a solution.

Q: The acid ionization constant for Al(H2O)63+(aq) is 7.9×10-6. Calculate the pH of a 0.0366 M solution…

A: Since you have posted multiple questions, the answer for first question is given below. Kindly…

Q: Calculate the pH of a solution containing 1 x 10-7 M of hydronium ions [H3O+]. pH = 5.0 pH = 6.0 pH…

A: Since the pH of any solution is given by  pH = -log[H3O+] where [H3O+] = concentration of H3O+ ions

Q: Calculate the Hydrogen ion concentration of nitric acid solution with a pH of 5.34 Round to 2…

A: Concentration of hydrogen ion = 4.57 × 10-6 mol/liter pH is the negative log of the molar hydrogen…

Q: Determine the pH and hydrogen ion concentration in a 0.1425M solution of ethylamine, C2H5NH2 at…

A: Here, we have to calculate the pH and hydrogen ion concentration in a 0.1425 M solution of…

Q: The pH of a human blood sample is 7.30. What is concentration of OH- in blood? a. 5.01 ×× 10-8 M…

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Q: 2)  Circle the phrase in parentheses which will make the statement correct. A solution with a pH of…

A: The pH of a particular substance is the negative logarithm of the (H+) hydrogen ion concentration.…

Q: Calculate the [OH−] and the pH of a solution with an [H+]=0.40 M at 25 °C. [OH−]= pH=   Calculate…

A: pH = -log [H+] [H+][OH-] = 10-14

Q: Calculate the pH of a 0.15 M solution of a basic solution of NH3. 2.Calculate the pH of a 0.10 M…

A: NH3 is a weak base.  H2S is a weak acid .

Q: Calculate the H3O+ concentration from each pH: (a) 2.42;    (b) 13.39.

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Q: Calculate the pH of 0.200 M HNO3(aq). 1.609 -1.140 0.699 2.000 13.800

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Q: Calculate the hydroxide ion concentration, [OH−]

A: Given :- pH = 7.38  To calculate :- concentration of hydroxide ions i.e. [OH-]  [H+].[OH-] = Kw  KW…

Q: If the pH of a solution increases from 3.1 to 5.1 the hydronium ion concentration decreases by a…

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Q: Suppose a 0.5 M solution of each of the compounds listed is prepared. Select all of the compounds…

A: A. Ba(NO3)2 on hydrolysis will produce Ba(OH)2 and HNO3.  Ba(NO3)2 + 2H2O = Ba(OH)2 + 2HNO3  As…

Q: Calculate the pH of a 0.600 M solution of methylamine CH3NH2.  Kb = 4.4 x 10–4

A: CH3NH2 is a base and CH3NH3+ is its conjugated acid. pKb of CH3NH2 is 4.4×10-4. Expression for Kb is…

Q: The hydronium ion concentration of a solution is 5.03×10+-2 M what is the pH A) 0.0503 B) 0.702 C)…

A: [H3O^+] = 5.03 × 10^-2M

Q: Determine the pH of a solution that is 0.00482 M HCl0.00482 M HCl and 0.0304 M HClO2. The Ka of…

A: Given -> Molarity of HCl = 0.00482 M Molarity of HClO2 = 0.0304 M Ka = 1.1 × 10-2

Q: Determine the ethylamine concentration of an aqueous solution that has a pH of 11.82. a)…

A: Given: pH = 11.82 Kb of ethylamine = 5.6×10-4

Q: Calculate the [OH−] and the pH of a solution with an [H+]=0.0027 M at 25 °C. [OH−]= pH=

A: we know that  at 25 °C        [H+] [OH−]  = 10-14               and    pH + pOH = 14   pH = - log…

Q: Calculate the pH for each H3O+ concentration.   [H3O+] = 1×10−7 M pH=     [H3O+] = 0.001 M pH=…

A: Answer:- This question is answered by using the simple concept of calculation of pH using the…

Q: What is the concentration of hydronium ion ([H3O+] in a solution with a pH of -1.3?   a. 0.050 M…

A: We have to calculate  the concentration of hydronium ion ([H3O+] in a solution with a pH of -1.3.

Q: he hydronium-ion concentration of a solution is 7.0 × 10-6 M. What is the solution pH? 2.00   6.36…

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Q: Explain why the pH of 0.1 M acetic acid (pH = 3) is higher than the pH of 0.1 M trifluoroacetic acid…

A: PH is defined as the negative logarithmic of concentration of hydronium ion

Q: 1)Why the PH start from 0 to 14 ? 2) why PH =14

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

Q: Stoli vodka has a [H+] of 1.6 x 10(-8). What is the pH of Stoli pH = -1(log[H+])

A: We know that pH is defined as the -ve log of the concentration of H+

Q: Calculate the pH of a 0.14 M solution of diethylamine

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Q: the pOH of the compound

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Q: Calculate the pH of a 0.0820 M propionic acid solution.     2.99     2.16     The answer is not…

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Q: pH

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Q: Calculate the pH of 10^-7 M H2SO4

A: Each mole of H2SO4 provide 2 moles [H+] ion.

Q: What is the pH of a 1.981.98 ×10−2×10-2 M solution of KOH?   12.312.3 3.873.87 6.986.98 1.701.70…

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Q: If the pH of a solution increases from 3.1 to 5.1 the hydronium ion concentration

A: Answer= Concentration decrease by 100

Q: The pH scale is a logarithmic scale. The acidity of a substance A is 2,000 times more acidic than a…

A: The pH scale is a logarithmic scale.  The acidity of a substance A is 2,000 times more acidic than a…

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.