If 175 mL of a 0.0208 M AgNO3 solution is added to a 250 mL 0.0380 M K2CrO4, will Ag+ precipitiate completely?

Q: OO O O O A 25.0-ml sample of 0.175 M C2H5NH2 is titrated with 0.150 M HCI. What is the pH at the…

A: Given,  Molarity of C2H5NH2 = 0.175 M  Volume of C2H5NH2 in mL = 25.0 mL  Molarity of HCl = 0.150 M…

Q: Calculate the molar solubility of Ag2SO4 in (a) 0.22 M AgNO3 and (b) 0.22 M Na2SO4.

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Q: What you expect to observe on mixing 0.1M AgNO3 with 6M NaOH. Will there be a color? Will bubbles…

A: Silver oxide - a displacement reaction occurs, but silver hydroxide isn’t thermodynamically stable…

Q: NaI crystals are slowly added to a solution that is 0.100M Pb(NO3)2 and 0.100 M AgNO3. Which vill…

A: When the ionic product of any salt becomes equal or greater than its solubility product then the…

Q: 50.0 mL of HCIO2 is titrated with 16.38 mL of 0.25 M NaOH before the color change of the endpoint…

A: 50.0 mL of HClO2 is titrated with 16.38 mL of 0.25 M NaOH before the color change of the enpoint…

Q: If exactly 1.00 liter of 2.0 M NH3 (final concentration) is required to dissolve 5.0 mmol of the…

A:

Q: 15.0 mL of 0.475M CH3COOH is titrated with 0.450 M RbOH. What is the pH after 18.0 mL of RbOH has…

A: Given: Concentration of CH3COOH= 0.475M Volume of CH3COOH=  15.0mL Concentration of RbOH = 0.450M…

Q: A 50.00 mL aliquot of 0.0100 M NH3 is titrated with 0.02136 M HCl. What is the pH of the solution at…

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Q: Calculate the concentration of buffer components present in 183.00 mL of a buffer solution that…

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Q: Calculate the pH for the titration of 50.0 mL of 0.1000 M Na2CO3 after addition of 49.00 mL of…

A: Msskns

Q: the 1.00 L buffer solution is 0.150 M in HC7H5O2 and .250 M in LiC7H5O2. calculate the pH of the…

A: We have to calculate the pH of buffer solution after HCl is added

Q: What volume of 0.2M HCI must be added to 250ml of 0.3M sodium mandelate to produce a buffer solution…

A: Given,  Molarity of HCl = 0.2 M  Molarity of sodium mandelate (say NaA) = 0.3 M Volume of sodium…

Q: The solubility product of Ag2CO3 is 8.1 ∙ 10^-12. H2CO3 is a weak acid. How is the solubility of…

A: The equation for the dissociation of Ag2CO3(s) is: Ag2CO3(s) + H2O(l)  <----> 2Ag+(aq) +…

Q: What you expect to observe on mixing 0.1M AgNO3 with HCl. Will there be a color? Will bubbles form?…

A: The question is based on qualitative analysis. we have to describe the observations..

Q: A 175 mL buffer solution is 0.177 M in HONH2 and 0.149 M in HONH3 CL What is the pH of the solution…

A:

Q: A 75.0-mLmL volume of 0.200 MM NH3NH3 (Kb=1.8×10−5Kb=1.8×10−5) is titrated with 0.500 MM HNO3HNO3.…

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Q: You titrated 1.0 mL of a saturated calcium iodate Ca(IO3)2 solution in 0.0100 M potassium iodate…

A: Since the  IO3- concentration coming from KIO3 solution = concentration of KIO3 solution This is…

Q: What is the molar solubility of PbBr2 in 0.500 M KBr solution?

A: Given: Concentration of KBr solution = 0.500 M Known: Ksp for PbBr2 = 6.60×10-6

Q: What masses of dimethylamine and dimethylammonium chloride do you need to prepare 3.00 L of pH =…

A: Given,  The volume of dimethyl amine and dimethyl ammonium chloride buffer = 3.00L The total…

Q: Which one of the following titrations is expected to have a pH < 7 at the equivalence point? A) HNO₃…

A: The right answer is option A) HNO₃ titrated with LiOH

Q: Calculate the pH of 100.0 mL of a buffer that is 0.0800 M  NH4Cl and 0.135 M  NH3 before and after…

A: NH4Cl is salt and NH3 is a base. pKa of NH3 = 4.75

Q: Calculate the molar solubility of BaF2 in a buffer solution containing 0.20 M HF and 0.20 M NaF.

A: Buffer solution is a solution of weak acid and its conjugate base or weak base and its conjugate…

Q: What is the maximum concentration of Ni²⁺ that can be added to a 0.00130 M solution of Na₂CO₃ before…

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Q: 3. Sketch a titration curve for the titration of 0.100 M NH3 (weak base) with 0.100 M HCI. Label the…

A: We have sketch the titration curve for titration of 0.100 M NH3 with 0.100M HCl.

Q: What is the maximum concentration of Ag+ that can be added to a 0.00250 M solution of Na2CO3 before…

A: The solubility product (Ksp) constant is the equilibrium constant for the dissolution of a solid…

Q: A 50.0 ml. sample of 0.15 M NH, is titrated with 0.10M HCI, Determine the equivalence point of this…

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Q: Calculate the molar solubility of PbCrO4 in 1.0 x 10-3M K2CrO4

A: Given data :

Q: What is the maximum concentration of Ag⁺ that can be added to a 0.00300 M solution of Na₂CO₃ before…

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Q: Calculate the molar solubility of CdCO3 in a buffer solution containing 0.115 M Na2CO3 and 0.120 M…

A:

Q: What is the maximum concentration of Ag+ that can be added to a 0.00110 M solution of Na₂CO3 before…

A: The question is based on the concept of solubility product principle.  It that states that when a…

Q: What is the maximum concentration of Ag+ that can be added to a 0.00650 M solution of Na₂CO3 before…

A: Answer: At the saturation point  ionic product of silver carbonate will become equal to its…

Q: The following pictures represent solutions of AgCl, which may also contain ions other than Ag + and…

A: When ions are in equal amount then equilibrium is attend.

Q: How many grams of sodium sulfate can be added to 595 mL of 1.6 x 10 M barium chloride before a…

A:

Q: c) A student titrated 50.0 mL of a 0.10 M solution of a certain weak acid with NaOH. The results are…

A: Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated…

Q: What is the pH after 20.0 mL of 1.0 M NaOH is added to a 1.0-L buffer solution composed of 0.50 M…

A: Step 1:Step 2:

Q: A buffer made up of equal volumes (396.8 mL) of each of 0.618 M A H and 0.857 M A minus. What is p H…

A: Given data,Molarity of AH=0.618MMolarity of A-=0.857MVolume of buffer=396.8mL=0.3968LMolarity of…

Q: Which of the following accurately describes the primary species in solution at point A on the…

A: In the given titration curve, HF is titrated with NaOH.

Q: A 26.6 mL sample of 0.365 M trimethylamine, (CH3)2N, is titrated with 0.397 M perchloric acid. The…

A:

Q: A sample of 0,444 M methylamine (CH3NH2, K 4.29 x 10-) is titrated with 0.444M HCL What is the pH at…

A: Whenver an acid and base reacts with each other than they form salt and water and the process is…

Q: A solution of 50.0 mL of 0.40 M NH3 is being titrated with a 0.40 M solution of the strong acid HCl.…

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Q: To confirm the presence of silver ion, HNO3 reforms a precipitate of AgCl because

A: Silver ions in solution can be identified by treating Ag(NH3)2+ with nitric acid.  If the solution…

Q: 16.57 If 20.0 mL of 0.10 M Ba(NO3)2 are added to 50.0 mL of 0.10 M Na₂CO3, will BaCO3 precipitate?

A:

Q: What is the pH of a nitrous acid/nitrite buffer that consists of 0.15 M HNO2 and 0.65 M LiNO2? What…

A: First calculate the pH.  Then calculate the pH of new solution.

Q: When a sparingly soluble salt like AgCl is added with HCl, what happens to its solubility?

A: AgCl (s)⇌ Ag (aq)   + Cl- (aq) HCl à H+ (aq)   Cl1-(aq)   HCl is a stong acid, it ionizes completely…

Q: A 45.00 mL sample of 0.35 M NH3 is titrated with 0.25 M NaOH. (Ka = 2.3 x 10^5) Calculate Kc

A: NH3 + NaOH ⇌ NaNH2 + H2O Kc = [NaNH2][H2O] / [NH3][NaOH] Next, we need to determine the initial…

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.