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 6.79? [HS¯] [H2S]

Q: How many grams of solid ammonium bromide should be added to 2.00 L of a 5.44×10-2 M ammonia solution…

A: pH is the negative logarithm of hydrogen ions. pH values vary from 0 to 14. O is very acidic while…

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: 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: A buffer that contains 0.17 M of a base, B and 0.28 M of its conjugate acid BH+, has a pH of 8.9.…

A: A buffer is a solution that can resist a change in pH when small amount of base or alkali is added…

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: How many grams of solid ammonium bromide should be added to 2.00 L of a 0.274 M ammonia solution to…

A: Given data, pH of the buffer=8.530 This buffer is basic buffer. So,pOH=14-pH =14-8.530=5.47…

Q: How many grams of solid ammonium chloride should be added to 2.00 L of a 0.211 M ammonia solution to…

A: For NH3 , pKb = 4.75  pOH = 14.00 - pH = 14.00 - 8.630 = 5.37 Henderson equation for basic buffer…

Q: How many grams of solid ammonium bromide should be added to 2.00 L of a 0.205 M ammonia solution to…

A: Given data :

Q: A buffer solution is prepared by dissolving  1.300 g  of ammonium chloride (NH4Cl) into  100.00 mL…

A: Mass of ammonium chloride is 1.3 g. Molar mass of ammonium chloride is 53.491 g/mol.

Q: 12:19 1 Jessica - Chemical Acid-Base Equilibria 回Q K = (b) Calculate the pH of 0.1mol dm potassium…

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Q: A buffer with a pH of 11.2 contains CH3NH2 and CH3NH3C1 in water. You may want to reference (Page)…

A: Given: pH of buffer = 11.2 pKb of CH3NH2 = 3.36 And the buffer solution is of CH3NH2 and CH3NH3Cl.

Q: A buffer is prepared by mixing 35.2 mL of 0.183  M NaOH with 141.2  mL of 0.231 M acetic acid. What…

A: Given: Concentration of acetic acid = 0.231 M Volume of acetic acid solution = 141.2 mL = 0.1412 L…

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 solution is made by dissolving 0.1283 g of the acid form of the buffer TRIS (molecular mass =…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: How many grams of solid sodium fluoride should be added to 1.50 L of a 0.169 M hydrofluoric acid…

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Q: Which of the following 1:1 mixtures would be best suited to form a buffer closest to a pH of 10 5? O…

A: SOLUTION: Step 1: The pH of a buffer solution can be calculated from the Pkb value as follows.…

Q: A buffer consists of 0.21 M H3PO4 and 0.38 M NaH2PO4. Given that the K values for H3PO4 are, Ka1 =…

A: Given that, a buffer is made by 0.21 M of H3PO4 and 0.38 M of NaH2PO4. The dissociation constant…

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

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Q: The titration curve of a weak acid, HnA has 3 inflection points at pH = 3.5, 6.7 and 10.3. If 0.1 M…

A:

Q: A buffer that contains 0.55 M of the base, B, and 0.35 M of its conjugate acid, BH+, has a pH of…

A: Given: The concentration of base, [B] = 0.55 M The concentration of conjugate acid, [BH+] = 0.35 M…

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: 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: You are creating 500.0 mL of a buffer that is 0.50 M in both HCIO and CIO-. What mass of KCIO must…

A: We have to calculate mass of KClO for the buffer solution

Q: A chemistry graduate student is given 300, ml. of a 1.00M nydrocyanic acid (HCN) solubon.…

A:

Q: A buffer is made from 25.0mL of 1.0M CH3COOH and 25.0mL of 1.0M CH3COONa, what would be the pH of…

A: Since moles = concentration X volume of solution in L  Hence the moles of CH3COOH taken = 1 X 25 /…

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: A buffer that contains 0.40 M base, B, and 0.25 M of its con-jugate acid, BH⁺, has a pH of 8.88.…

A: Given data: Molarity of base B = 0.40 M Molarity of its conjugate acid BH+= 0.25 M pH = 8.88 Using…

Q: The pK, value for H2S is 7.00. What mole ratio of KHS to H2S is needed to prepare a buffer with a pH…

A: The henderson hasselbalch equation for weak acid, pH = pKa + log [conjugate base][acid]

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 that is 0.397 M in HCN and 0.397 M in KCN has a pH of 9.40. The addition of 0.01…

A: Given that, We have a buffer solution containing 0.397 (M) HCN and 0.397 (M) KCN. The buffer…

Q: A buffer with pH of 4.74 is composed of 0.50mol sodium acetate and 0.60mol acetic acid is diluted to…

A: In this question, we will determine the moles of NaOH which is added to given buffer solution.  You…

Q: How many grams of solid potassium cyanide should be added to 1.50 L of a 0.217 M hydrocyanic acid…

A: We would use hende Hasselbalch to to calculate the grams of potassium cyanide needed.

Q: Calculate the pH of a buffer solution containing 0.92 M NaF and 0.44 M HE. The pKa of HF is 3.14.

A: Given that : Concentration of NaF = 0.92M Concentration of HF = 0.44M pKa = 3.14 pH of the buffer…

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: 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: A buffer contains 0.15 mol of propionic acid (C2H5COOH)and 0.10 mol of sodium propionate (C2H5COONa)…

A: A solution of propionic acid and sodium propionate form a buffer solution therefore a solution…

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

A:

Q: A buffer consists of 0.12 M NaH2PO4 and 0.33 M Na2HPO4. Phosphoric acid is a triprotic acid…

A: Given as Ka1 = 7.2 × 10−3,  Ka2 = 6.3 × 10−8, Ka3 = 4.2 × 10−13 The most important Ka value…

Q: How many grams of solid ammonium chloride should be added to 2.00 L of a 0.282 M ammonia solution to…

A:

Q: Acetic acid (molecular weight = 60.05 g/mol) and sodium acetate (molecular weight = 82.03 g/mol) can…

A: Initial number of moles of NaOH, acetic acid and sodium acetate is determined as follows, 1 mL =…

Q: pH of a buffer solution prepared by mixing 20 mL of 1 M NH4OH and 40 mL of 2 M NH4CI will be (pKp of…

A: Given data  Buffer solution has 20 mL of 1 M NH4OH40 mL of 2 M NH4Cl pKb = 4.7   for NH4OH…

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: How many moles of CH;NH;CI need to be added to 200.0 mL of a 0.500 M solution of CH3NH2 (Kb for…

A: The solution is a buffer solution of weak base CH3NH2 and its conjugate acid CH3NH3Cl.

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…

Q: What is the pH of a buffer composed of 0.45 M C5H10NH and 0.65 M [C5H10NH2]Cl?

A: Formula for calculating pOH of a solution consisting of a weak base and its salt with a strong acid:…

Q: A buffer solution is prepared by mixing 20.0 mL 0.45 M CH3COOH (acetic acid) with 35.0 mL 0.45 M…

A: Moles of acidic part of the buffer, CH3COOH added = C*V= 0.45 molL*20.0 mL * 1 L1000 mL= 0.009 mol…

Q: How many grams of solid ammonium chloride should be added to 2.00 L of a 0.203 M ammonia solution to…

A: Given,  The mass of solid ammonium chloride should be added to 2.00 L of a 0.203 M ammonia solution…

Q: How many grams of sodium hypochlorite, NaCIO, need to be added to 227 mL of a 0.185 M solution of…

A:

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.