The pK, value for H2S is 7.00. What mole ratio of KHS to H2S is needed to prepare a buffer with a pH of 6.68? (HS ] [H2S]

Q: A beaker with 2.00x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The…

A: The ratio of acetate ion and acetic acid in the given buffer solution can be calculated using…

Q: The molar solubility of lead carbonate in a 0.251 M ammonium carbonate solution is M.

A: Given that:  Concentration of ammonium carbonate [(NH4)2CO3] = 0.251M (NH4)2CO3(aq) <....>…

Q: What is the molar solubility of FeCl3FeCl3 in water?

A:

Q: Calculate the weight of natrium acetate you would need to make 100 mL of a 0.1M solution. Weigh out…

A: Given: Volume of natrium acetate = 100 mL Molarity of natrium acetate = 0.1 M Molar mass of natrium…

Q: Write a solubility equillibria equation of the precipitation of Ag+ with ammonia.

A: When ionic product of  a compound exceeds value of Ksp the the compound at a definite temperature…

Q: What is the maximum volume of 2.4 M N2OH(aq) that the buffer (pH=5.75) prepared from sodium acetate…

A: Given: The value of pH of the buffer solution is 5.75 The volume of acetic acid is 2.5 L The…

Q: Calculate the solubility of CaC2O4 in a solution containing 0.001 molarity H+

A: Solubility indicates the maximum amount of a substance that can be dissolved in a solvent at a given…

Q: A buffer can be prepared from a weak acid, HA, and it's conjugate base, A⁻. A 1L solution is…

A: Given data,[HA]=0.2M[A-]=0.1MpKa=7.5Molarity of KOH=1MVolume of KOH=50mL0.05LVolume of buffer=1L

Q: A buffer solution with a pH of 3.86 is prepared with 0.50 M formic acid and M sodium formate. The K,…

A: The formula of pH of a buffer solution is: pH=pKa+log[Salt][Acid]

Q: Determine the pH of the buffer solution produced by the reaction of 5mL 0.1 M KOH and 30 mL 0.1 M…

A: Given-> Volume of KOH = 5 ml Molarity of KOH = 0.1 M Volume of CH3COOH = 30 ml Molarity of…

Q: A buffer containing NH3(aq) and NH4Cl(aq) has a pH of 9.5. What is the [NH3]/[NH4+] ratio in this…

A: We know that,       According to Henderson-Hasselbalch equation:           pH =pKa + log [ salt ] /…

Q: A buffer is made up from 0.15 M acetic acid and 0.5 M sodium acetate. What is the pH of the buffer…

A:

Q: What is the molar solubility Sn (OH)2 of in a buffer solution containing equal concentrations of NH3…

A: Here we have to determine the solubility of Sn(OH)2 in a buffer of solution containing equal…

Q: What is the molar solubility of Sn(OH), in a buffer solution containing equal concentrations of NH,…

A: 1.) To calculate solubility of Sn(OH)2 in buffer solution , we would first calculate pOH if buffer…

Q: The solubility of PbBr2 is O.427 g per 100 ml (367.008 g/mol) of solution at 25 C, determine the…

A: Given that the solubility of PbBr2 is 0.427 g per 100 ml and have a molar mass of 367.008 g/mol at…

Q: Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of…

A: Given   The volume of CH3COOH solution is 500.0 mL. The molarity of CH3COOH solution is 0.200 M. The…

Q: A maximum of 0.50 g of CuX(100 g/mol)will dissolve in 100 mL of a 1.0M ammonia buffer (total…

A:

Q: What is the molar solubility of Ag₂CrO₄?

A: Here we are required to find the solubility of silver chromate.

Q: When K2(S) is added to a saturated solution of FeS , what happens to the solubility of FeS

A: We have to predict about solubility of potassium sulfide.

Q: The molar solubility of calcium fluoride in a 0.297 M ammonium fluoride solution is M.

A:

Q: Write the solubility product constant for: A. BaCrO4 B. Ag2CrO4 C. Mg3(PO4)2

A:

Q: What is the molar solubility of AgSCN in a solution that is buffered to pH 1.007 The Ksp of AgSCN is…

A: The solubility reaction of AgSCN can be written as, => AgSCN (s) -------> Ag+ (aq) + SCN- (aq)…

Q: The molar solubility of silver chromate in a 0.215 M ammonium chromate solution is __________M.

A:

Q: What will be the pH if 5.00 grams of solid KOH is added to 500 mL of a solution containing 0.020…

A: Since you have posted 2 completely unrelated questions, we are entitled to answer only the first.

Q: How many grams of solid ammonium chloride should be added to 2.00 L of a 0.172 M ammonia solution to…

A: It will form a basic buffer. And pkb for NH3 = 4.74 Molar mass of Ammonium chloride is 53.49 g/mol

Q: 5. A solution of 0.09 M in Mg²+ and 0.33 M in NH.. What minimum concentration of NH, will cause…

A:

Q: 4. A buffer is prepared containing 1.00 M acetic acid and 1.00 M sodium acetate. What is its pH?

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: A buffer solution that is 0.470 M in HClO and 0.470 M in KCIO has a pH of 7.46. The addition of 0.01…

A:

Q: The molar solubility of barium chromate in a 0.229 M barium acetate solution is  M

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

Q: A beaker with 2.00x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The…

A: The chemical equation can be written as: Given data is: Initial pH = 5.00 Initial volume of acetic…

Q: A buffer solution contains 0.471 M KHCO, and 0.349 M Na,CO3. Determine the pH change when 0.106 mol…

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

Q: A buffer solution is created containing 3.25 M acetic acid and 0.550 M sodium acetate. The Ka of…

A: Given :-  [CH3COOH] = 3.25 M  [CH3COONa] = 0.550 M  Ka for acetic acid = 1.77 x 10-5  To calculate…

Q: How many grams of (CH3)2NH2CI must be added to 1.00 L of 0.200 M (CH3)2 NH to produce a buffer with…

A: Given : Concentration of (CH3)2NH = 0.200 M Volume of buffer solution = 1.00 L pH of buffer = 10.65…

Q: The composition of a hydrated sodium-salt of a chromium(III)-oxalate complex ion conforms to the…

A:

Q: Calculate the pH of a buffer made up of 0,500M NH, and 0.456M NH,CI, pKb NH, = 4.74. %3D

A: Given:  [NH3] = 0.500 M  [NH4Cl] = 0.456 M  pKb(NH3) = 4.74  Since above solution contains weak base…

Q: What is the molar solubility of FeCl3 in water?

A: Given :-  The given salt is FeCl3  Molar solubility of FeCl3 in water = ?…

Q: A buffer contains 0.10 mol of acetic acid and 0.13 mol ofsodium acetate in 1.00 L. (a) What is the…

A: The pH of a Acidic buffer can be calculated by the Henderson Hasselbalch equation:            pH=pKa…

Q: The ?spKsp of PbBr2PbBr2 is 6.60×10−6.6.60×10−6. What is the molar solubility of PbBr2PbBr2 in pure…

A: The solubility reaction of PbBr2 is  => PbBr2 (s) -----> Pb2+ (aq) + 2 Br- (aq)

Q: A buffer is created by adding 0.125 moles of hypobromous acid (HOBr, pKa = 8.65) and 0.475 moles of…

A:

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A: At 22 degree Celsius PH + POH = 14

Q: 4. Two RND Engineers were assigned to create buffer solutions for two separate product lines that…

A: We need to prepare buffer solutions and need to calculate pH and need to maintain it so that it…

Q: A buffer that contain 0.40 M of a base, B, and 0.25 M of its conjugate acid, BH+, has a pH of 8.88.…

A: Given:             Initial concentration of Base [B] = 0.40M   Initial concentration of Conjugate…

Q: A solution is initially 0.0380 M in Fe3+ and 0.29 M in NaCN. If the Kf for the complex ion Fe(CN) is…

A:

Q: The buffers had a strong base added so that they both reach equivalence point. Buffer F has 100mL of…

A: The buffer capacity is the moles of either strong acid or strong base which are mainly needed to…

Q: A buffer solution is made that is 0.323 M in H2CO3 and 0.323 M in NaHCOз. If Kal for H2CO3 is 4.20 ×…

A: The concentration of H2CO3 and NaHCO3 in buffer solution is 0.323 M. The first dissociation constant…

Q: Consider the titration of 15.75 mL of 0.549 M potassium propanoate, CH3CH;CO,K, with 0.207 M HNO3.…

A: Given : Concentration of CH3CH2CO2K = 0.549 M Volume of CH3CH2CO2K solution = 15.75 mL = 0.01575 L…

Q: A buffer that contains 0.578 M base, B, and 0.299 M of its conjugate acid, BH*, has a pH of 9.09.…

A:

Q: A buffer is made up of equal volumes of 0.1 M weak acid (AH) and 0.1 M conjugate base (A minus). The…

A: Given :- concentration of weak acid i. e. [HA] = 0.1 M  Concentration of conjugate base i. e.  [A-]…

Q: A buffer that contains 0.405 M base, B, and 0.296 M of its conjugate acid, BH", has a pH of 9.13.…

A: From Henderson Hasselbalch equation: pH=pKa+logconjugate baseacid Given, [B] is 0.405 M, [BH+] is…

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.