A 21.6 mL sample of 0.350 M dimethylamine, (CH3),NH, is titrated with 0.235 M hydrochloric acid. After adding 50.8 mL of hydrochloric acid, the pH is

Q: The molar solubility of lead chromate in a 0.250 M ammonium chromate solution is

A:

Q: A 20.6 mL sample of 0.377 M methylamine, CH3NH2, is titrated with 0.364 M perchloric acid. After…

A: Number of moles of   CH3NH2= M*V = 0.377 M* 20.6 mL = 7.7662 mmol Number of moles of HClO4 = M*V =…

Q: The solubility of Mg(OH)2 in a particular buffer solution is 0.66 g/L. Part APart complete What must…

A: Solubility product(Ksp) Solubility product is the concentration equilibrium of the saturated…

Q: Define the term selective precipitation?

A: Given term,           Selective precipitation

Q: A 10.00mL sample of 0.15 M of chlorous acid, HClO2 (aq) is titrated with 0.20 M sodium hydroxide,…

A: The dissociation of Chlorous acid (HClO2) is represented as:HClO2 (aq) ⇌  H+ (aq) + ClO2- (aq)Ka =…

Q: A 27.6 mL sample of 0.275 M methylamine, CH3NH2, is titrated with 0.275 M hydroiodic acid. After…

A: The reaction will be as follows: HI(aq) + CH3NH2 ---------> CH3NH3+(aq) + I-(aq). The volume of…

Q: Write the solubility product expression for copper (II) hydroxide, Cu(OH)2?

A: The solubility reaction of Cu(OH)2 is given by  => Cu(OH)2 (s) --------> Cu2+ (aq) + 2 OH-…

Q: The molar solubility of calcium fluoride in a 0.274 M calcium acetate solution is ______M.

A:

Q: A buffer solution contains 0.420 M NaHCO3 and 0.262 M Na2CO3. If 0.0303 moles of potassium hydroxide…

A: Initially, the solution contains a weak acid (NaHCO3) and its salt with a strong base (Na2CO3).…

Q: A 28.4 mL sample of 0.366 M ethylamine, C2H5NH2, is titrated with 0.395 M hydrobromic acid. After…

A:

Q: The solubility product for calcium hydroxide is 6.5 x 10−6.  What is the pH of this solution?

A:

Q: A 100.0 mL solution of 0.135 mol/L Hydrobromic Acid, HBr, is being titrated with 0.365 mol/L…

A: Given the value  Volume of HBr = 100.0 mL  Concentration of HBr = 0.135 mol/L  Volume of KOH = 80.0…

Q: The molar solubility of nickel(II) sulfide in a 0.193 M ammonium sulfide solution is

A:

Q: The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as…

A: In the titration of weak acid with strong base, the pH of the solution is 7 when base is not added…

Q: Solid ammonium sulfide is slowly added to 125 mL of a 0.0634 M copper(Il) acetate solution. The…

A:

Q: Lactic acid is a monoprotic acid with the formula C3O3H6. You have a  25.00 mL  sample of lactic…

A: The concentration of acids is determined by a neutralization reaction with a base of known…

Q: The molar solubility of barium fluoride in a 0.142 M ammonium fluoride solution is М.

A:

Q: Calculate the minimum pH needed to precipitate Mn(OH)2so completely that the concentration of Mn2+…

A: The reaction can be written in following manner: Here, the solubility product factor works. The…

Q: If 0.02 M of NaOH will be added to the buffer solution prepared by mixing 0.215M sodium acetate and…

A: Given sodium acetate solution is 0.215 M and given acetic acid solution is of 0.125 M. When NaOH…

Q: The molar solubility of silver sulfide in a 0.134 M potassium sulfide solution is ______  M.

A:

Q: A solution is formed by adding 3.20 grams of solid sodium hypochlorite, NaClO, to 500.0 ml of…

A: Answer: Solution will be basic due to hydrolysis of hypochlorite ion because it is the conjugate…

Q: A 27.6 mL sample of 0.275 M methylamine, CH3NH2, is titrated with 0.275 M hydroiodic acid. After…

A: This question can be solved using Henderson-Hesselbech equation as:

Q: In a precipitation titration of 46.00 mL of a chloride solution of unknown concentration, 31.00 mL…

A: In  precipitation titrations, the stoichiometric reaction is a reaction which produces in solution a…

Q: The molar solubility of copper(II) sulfide in a 0.135 M sodium sulfide solution is

A: Ksp of CuS = 6.0 x 10-37 Concentration of Na2S = 0.135 M

Q: Solid silver fluoride is slowly added to 50.0 mL of a 0.252 M sodium sulfide solution until the…

A:

Q: A 23.1 mL sample of 0.372 M ammonia, NH3, is titrated with 0.354 M perchloric aci After adding 9.93…

A: Kb of NH3 = 1.8*10-5        [source : google]   millimoles of NH3 = molarity*volume = 0.372*23.1 =…

Q: The pH of a saturated solution of a metal hydroxide M(OH)2 is 10.500. Calculate the Ksp for this…

A: ksp : sloublity product Ksp = equilibrium between solids and  liquids

Q: What is the molar solubility of silver chloride in 0.65 M NH3(aq)? Solubility

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

Q: The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as…

A:

Q: A 23.1 mL sample of 0.382 M ethylamine, C,H;NH,, is titrated with 0.297 M hydrobromic acid. The pH…

A:

Q: The molar solubility of magnesium fluoride in a 0.174 M sodium fluoride solution is М.

A:

Q: A 25.5 mL sample of 0.362 M triethylamine, (C2H5)3N, is titrated with 0.285 M hydroiodic acid.…

A: Given data,Molarity of triethylamine=0.362MVolume of triethylamine=25.5mL=0.0255LMolarity of…

Q: The molar solubility of barium fluoride in a 0.257 M potassium fluoride solution is М.

A:

Q: A 21.0 mL sample of 0.308 M methylamine, CH3NH2, is titrated with 0.245 M hydrobromic acid. At the…

A: The question is based on the concept of titrations. we have been given a weak base and a strong…

Q: A 29.5 mL sample of 0.258 M ethylamine, C2H5NH2, is titrated with 0.340 M hydrochloric acid. After…

A: Given- Volume of ethylamine=29.5mL  Concentration of ethylamine =0.258M Volume of hydrochloric acid=…

Q: A 26.9 mL sample of 0.375 M diethylamine, (C2H5)2NH, is titrated with 0.258 M Hydrochloric acid.…

A: Given : Concentration of (C2H5)2NH = 0.375 M Volume of (C2H5)2NH solution = 26.9 mL = 0.0269 L…

Q: What is the pH of a saturated solution of magnesium hydroxide (the active ingredient in the antacid…

A: Milk of magnesia which is a saturated solution of magnesium hydroxide has a pH of  about 10.0 (basic…

Q: A 26.0 ml sample of 0.317 M triethylamine, (C,H5);N, is titrated with 0.293 M hydrochloric acid. The…

A: Given: Concentration of weak base triethylamine (Assuming B) = 0.317 M

Q: A 21.7 mL sample of 0.303 M methylamine, CH3NH2, is titrated with 0.209 M hydroiodic acid. After…

A: The above given problem can be solved using Henderson-Hesselbalch equation for weak base and strong…

Q: The molar solubility of manganese(II) sulfide in a 0.190 M sodium sulfide solution is М.

A: The ICE table and the molar solubility of the manganese (II) sulfide (MnS) in sodium sulfide (Na2S)…

Q: Explain the role of a buffer, such as an antacid table or sodium bicarbonate, on the pH of a…

A: The antacids play an important role in controlling the pH of the body solution (like blood).…

Q: A 22.6 mL sample of 0.318 M dimethylamine, (CH3)2NH, is titrated with 0.265 M hydrobromic acid.…

A: First we would write a reaction between given compounds . Then using moles of each compound , we…

Q: Can HCl, a strong acid, be added to pure water and there be no significant change in pH?

A: Addition of strong acid HCl will leads to dramatic change in pH.  When a strong acid HCl adds to…

Q: The molar solubility of barium phosphate in a 0.212 M ammonium phosphate solution is

A: Ba3(PO4)2(s)   <--------->  3Ba2+(aq)+2 PO43-(aq) The solubility product constant, Ksp is the…

Q: A 27.8 mL sample of 0.387 M trimethylamine, (CH3)3N, is titrated with 0.315 M hydroiodic acid. After…

A:

Q: A 26.9 mL sample of 0.348 M ethylamine, C2H5NH2, is titrated with 0.391 M hydrobromic acid.…

A: The pH of a solution formed by the mixture of a weak base and its conjugate acid can be calculated…

Q: Calculate the molar solubility of Mg(OH)2 in 1.00 M NH4Cl (aq).

A: Considering Ksp Mg(OH)2 = 1.8×10-11 and  Kb (NH3) = 1.8 × 10-5 AND THEN SOLVING THE QUESTION Mg(OH)2…

Q: A 24.9 mL sample of 0.234 M ethylamine, C,H5NH,, is titrated with 0.315 M hydroiodic acid. After…

A: Value of pH is used to measure the acidity or basicity of a solution. At room temperature, pH of a…

Q: A 26.8 mL sample of 0.345 M triethylamine, (C,H;);N, is titrated with 0.217 M perchloric acid. At…

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.