584.0 mL of a 0.13 M solution of ammonia is mixed with 584.0 mL of a 0.13 M solution of HBr. What is the pH of the resulting solution of NH Br? (Ko for NH3 equals 1.8 x 105) pH =

Q: What is the number of moles of 10.0 g NH₄Cl?  What is the molar concentration of NH₄Cl?  What is…

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Q: The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of…

A: Given:Ka of H2CO3 is 4.4 ✕ 10−8

Q: 3. (a) A 20.0 mL sample of 0.200 M cyanic acid (HOCN, K₁=3.3 x 104) is titrated with 0.400 M NaOH.…

A:

Q: A 0.21-mol sample of a diprotic acid, H2A, is dissolved in 250 mL of water. The Ka1 of this acid is…

A: Given that: Moles of diprotic acid, H2A = 0.21 mol Volume = 250 mL = 0.250 L   (use 1 L = 1000 mL)…

Q: Lareina the laboratory technician is given the task of making a solution containing HOBr…

A:

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: The compound methylamine is a weak base like ammonia. A solution contains 0.263 M CH,NH3* and 0.204…

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Q: A solution of hydrobromic acid has [HBr] = 1.3×10-2 M. What is the pH of this solution

A: As per guidelines if multiple questions, first question is allowed to answer, please post  questions…

Q: The hydrogen ion concentration s 37.93% greater than the hydro

A: As we know pH = -log [H+] If we know the concentration of Hydrogen ion of solution B we can find the…

Q: If a buffer solution is made from 300.0 mL of 2.2 M pyridine salt mixed with 350.0 mL of 2.0 M…

A: Buffer solution pH is determined using Henderson–Hasselbalch equation. Which relates salt…

Q: The hydrogen ion concentration of a fruit juice is 3.3 x 10-2 M. What is the pH of the juice? Is it…

A: Given, [H+] = 3.3 x 10-2 M  PH is defined as negative logarithm of concentration of hydronium ion.

Q: Each of these three molecules contains an OH group. When dissolved in water one solution has a pH7.…

A:

Q: 6) 20.0 mL of a strong acid, HA, has a pH of 5.00. A) What would happen to the pH if 180.0 mL of…

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Q: A laboratory technician wants to determine the aspirin content of a headache pill by acid-base…

A: a. Given information: Concentration of HA = 0.015 M Ka of aspirin= 3 ×10-4

Q: Lareina the laboratory technician is given the task of making a solution containing HOBr…

A:

Q: 546.0 mL of a 0.13 M solution of ammonia is mixed with 546.0 mL of a 0.13 M solution of HBr. What is…

A: The question is based on the titrations.  we are titrating a strong acid hydrobromic acid with a…

Q: Lareina the laboratory technician is given the task of making a solution containing HOBr ( Ka = 2.8…

A:

Q: The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used…

A: The question is based on the concept of titrations. We have to calculate molarity of the acid and Ph…

Q: Calculate the pH of each of the following buffered solutions. Ka (HC2H3O2) = 1.8 × 10-5 1. 0.11 M…

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Q: You are running a titration. You have placed 40.0 mL of 0.200 M chlorous acid, HCIO2, in a flask and…

A: mmoles of HClO2 = 40 x 0.2 = 8 mmoles  mmoles of KOH = 80 x 0.1 = 8 mmoles  KOH + HClO2 ----->…

Q: 5.) A typical aspirin contains 324 mg of aspirin (HC,H,O4) with Ka = 2.8 x 104. If you dissolve two…

A: pH = -log[H+] Aspirin is a weak acid. For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molar…

Q: -5 A chemistry graduate student is given 125. mL of a 0.80M ammonia (NH3) solution. Ammonia is a…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: ne acidity of a solution is measured by its pH. H+ represents the concentration of hydrogen ions (in…

A: pH is defined as pH=-log[H + ]

Q: Chemistry The label of an energy drink states that it contains approximately 80 mg of caffeine…

A: Molecular weight of caffeine = 8×12+10×1+4×14+2×16=194 g/mol Weight of caffeine = 80 mg = 80×10-3g…

Q: 5 A chemistry graduate student is given 450. mL of a 0.10M ammonia (NH3) solution. Ammonia is a weak…

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Q: Red cabbage juice is a sensitive acid-base indicator; its colors range from red at acidic pH to…

A:

Q: 2) A buffer solution contains 0.339 M ammonia. If 0.0248 moles of hydrochloric acid are added to…

A:

Q: What is the pH of the solution containing 0.20 M NH3 and 0.15 M NH4Cl?

A: In an aqueous solution that consist of a mixture of the conjugate base of a weak acid along with the…

Q: Calculate the pH of each of the following buffered solutions. K₂ (HC₂H₂O₂) = 1.8 x 10-5 1. 0.19 M…

A: The pH of mixture of weak acid and its salt can be calculated using the formula:

Q: 4. How does the pH of each of the following solutions change when 5.0 mL of 1.0 M NaOH (a strong…

A: Number of moles of NaOH = M*V = 1.0 M * 5.0 mL = 5 mmol (1)Volume of water = 100.0 mL   pH of pure…

Q: 33. Consider a buffer solution that contains 0.45 M HCOOH and 0.55 M NaHCOO. Note that the Ka for…

A: Given: The concentration of HCOOH and NaHCOO in the buffer solution is 0.45 M and 0.55 M,…

Q: 1. If 30.00 ml of a 0.300 mol/L of a weak acid, CH,CO,H (aq), is titrated with a 0.300 mol/L…

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Q: A Titration of 10.0 mL of 0.15 M NaOH is added 0.35 M HNO3. What is the volume of HNO3 to reach…

A: 1) The volume of HNO3 to reach the equivalence point is 4.28 mL.2) pH = 5.74Explanation:1) Volume of…

Q: A conjugate acid (HA) and its conjugate base (A") is mixed to make buffer solutions. When 0.50 mol…

A:

Q: Lareina the laboratory technician is given the task of making a solution containing HOBr…

A: To calculate moles of each first.  Then to calculate pH.

Q: The acidity of a solution is measured by its pH. If H+ represents the concentration of hydrogen ions…

A: Given that :  pH of solution B = 3.4  using pH = -log[H+]  [H+] = 10-pH = 10-3.4 = 3.98 × 10-4 M So,…

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.