what volume of Boric acid 0.1 M and what volume of sodium hydroxide 0.1 M should be added together to produce a solution (buffer) with a pH of 9.1? (ka=6.0*10-10) 4H3BO3 +2NaOH --> Na2B4O7 +7H2O

Q: What would be the pH values when (a) 0.0090 mol HCI and (b) 0.0090 mol NaOH, added to 0.300 L of a…

A: Given(a): Concentration of HCl = 0.0090 Mb): Concentration of NaOH = 0.0090 MConcentration of Volume…

Q: Which of the following acids should be used to prepare a buffer with a pH of 3.4? CH3COОН, Ка - 1.8…

A:

Q: 13. 30 ml of 0.20 M NH,OH & 25 ml of 0.20 HCl are mixed. What is the pH? K = 1.8 X 10% Calculate the…

A: NH4OH is weak base and when it combines with limiting strong acid, HCl then a basic buffer is…

Q: Calculate the [OH-] of 101.40 mL of a buffer initially consisting of 0.1271 M C5H5N and 0.0838 M…

A:

Q: Acetic acid has a Ka of 1.8×10−5. a.) What is the pH of a buffer solution containing 0.20 M HC2H3O2…

A: Concentration of acetic acid[C2H3O2] = 0.20 MConcentration of acetate ion = 0.13 MKa = 1.8*10-5pH =…

Q: What ratio of NaCN to HCN is needed to prepare a pH 10.10 buffer? (Ka of HCN is 4.9 × 10¯1º)

A: The given data contains, pH = 10. Ka=4.9×10-10

Q: Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 59.5 mL…

A:

Q: A buffer solution is prepared by dissolving 0.200 mol of NaH2PO4 and 0.100 mol of NaOH in enough…

A: pH is used to determine the concentration of hydronium ion.

Q: What ratio of NaCN to HCN is needed to prepare a pH 9.90 buffer? (Ka of HCN is 4.9 × 10-10)

A:

Q: 1. 50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the…

A: Since you have posted multiple questions, we are entitled to answer the first only. 1) Given:…

Q: What is the pH (in two decimal places) of a weak base-strong acid titration when 25.0 mL of 0.56 M…

A: Volume of NaOCl = 25.0 mlMolarity of NaOCl = 0.56 MVolume of HCl = 23.0 mlMolarity of HCl = 0.34 MKa…

Q: Suppose you wanted to make a buffer of exactly pHpH 7.00 using KH2PO4KH2PO4 and Na2HPO4Na2HPO4. If…

A: Henderson – Hasselbalch equation can be used here, i.e pH=pKₐ+log₁₀([A⁻]/[HA])

Q: What is the pH of the buffered created by dissolving 60.0g HCN (MM= 27.0253 g/mol) and 60.0g KCN…

A: The PH can be calculated as follows

Q: (a) What is the pH of this buffer solution? (b) If 0.005 mol NaOH is added to 0.500L of this buffer…

A: pH can be calculated by using Henderson Hasselbalch equation  pOH = pkb + log ([salt]/[base]) pH =…

Q: Which of the following combination can be used to prepare a buffer with a pH of 3?     NaH2PO4 and…

A:

Q: Calculate the pH of a buffer solution made by mixing a 0.37 M formic acid (HCOOH) with 0.23 M sodium…

A: pH of buffer solution=3.54Explanation:So,pH of buffer solution=3.54

Q: Suppose you want to make a buffer with a pH of 6.90. Which of the following acid/conjugate base…

A: The pKa value can be used to predict the pH of the buffer solution and hence the suitable conjugate…

Q: What is the pH of a buffer that has 0.150 mol HC2H3O2 and 0.120 mol NaC2H3O2 in 2.00 L that has…

A:

Q: ming equal concentratic JO suope N2OCI / HOCI (K a= 3.2 x 10-8) NH 3/ NH 4CI (K a=5.6 x 10-10) NANO…

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

Q: What is the pH of a weak base-strong acid titration when 20.0 mL of 0.56 M of NaOCl (Ka = 3.0*10-8)…

A:

Q: A bottle with 0.5 L of ammonia (NH3) solution that is 13.2% by mass has a density = 0.9430 g/mL. How…

A: Given, Volume of ammonia solution =0.5L Density of ammonia solution = 0.9430g/mL Mass % of ammonia…

Q: Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 71.4 mL…

A: Note: Since you have posted a question with multiple sub-parts, we will provide the solution only to…

Q: Calculate the pH at the equivalence point in titrating 0.072 M solutions of each of the following…

A: (a) Hydrobromic acid (HBr): Reaction at equivalence point: HBr+NaOH→NaBr+H2​O pH=7.0 (neutral) (b)…

Q: A buffer is prepared by adding 150mL of KOH 1.00M to 250mL of H2PO4 1.00M. Calculate the moles of…

A: In the given question we have to calculate the mole of HCl that will be addade to this system to…

Q: A student titrates 20.00 mL of 0.300 M HCN (Ka of HCN = 4.9x10^-10) with 0.200 M NaOH. What is the…

A: When the moles of NaOH added are less than the moles of weak acid present, it will neutralize a part…

Q: What ratio of NaCN to HCN is needed to prepare a pH 9.80 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰)

A: Given data is as follows: The pH of the buffer solution = 9.80 The Ka of HCN = 4.9×10-10 The ratio…

Q: A buffer solution is made that is 0.445 M in HF and 0.445 M in NaF . (1) If Ka for HF is 7.20×10-4,…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: Calculate the pOH of 103.16 mL of a buffer initially consisting of 0.1752 M H2NCH2COOH and 0.1573 M…

A:

Q: How many millilitres of a 0.1 M solution of NaF and of 0.1 M solution of HF must be mixed to obtain…

A: Acidic buffer :-  A mixture of weak acid and its salt with strong base is known as acidic buffer For…

Q: What ratio of NaCN to HCN is needed to prepare a pH 9.50 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰)

A: The objective of this question is to find the ratio of sodium cyanide (NaCN) to hydrogen cyanide…

Q: Aspirin (C 9H 8O 4) is a weak monoprotic acid (K a = 3.3 x 10-4). You are analyzing a sample for a…

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

Q: Suppose you need a buffer with a pH of 4.9. Which conjugate acid-base pair should you use? O sodium…

A: To find the appropriate buffer of given solution we need to find the buffer range of each conjugate…

Q: A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is…

A:

Q: Consider a buffer made from 255 mL 0.10 M HC2H3O2 and 125 mL 0.10 NaC2H3O2. Ka for HC2H3O2 is 1.8 x…

A: Moles of HC2H3O2 = Molarity × Volume                               = 0.10 M ×0.255 L Moles of…

Q: Calculate the pH of a buffer made up by adding 0.65 mol of NaC2H3O2 (sodium acetate) to 00L of a…

A:

Q: Determine the pH during the titration of 21.0 mL of 0.446 M hypochlorous acid (K₂ = 3.5x10-8) by…

A: we have to calculate the pH of solution

Q: Calculate the pH of a buffered solution that is prepared by dissolving 0.3mol of NaHCO3 and 0.45mol…

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

Q: What volume of 2.00 M NaOH must be added to 150.0 mL of 1.50 M lactic acid to produce a buffer…

A: Given: pH of solution = 4.00 Concentration of NaOH = 2.00 M Ka of lactic acid = 1.38 × 10-4…

Q: 1. 50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the…

A:

Q: what is the (HSO4)-, (SO4)2- and ph of a buffer solution which is composed of 50mL of 0.25M NaHSO4…

A: We have to calculate the pH of the buffer solution

Q: What ratio of NaCN to HCN is needed to prepare a pH 10.10 buffer? (Ka of HCN is 4.9 × 101º)

A: HCN=acid NaCN =salt Buffer solution A buffer is a solution can ability to resist pH change upon the…

Q: 7. The pH titration curve of a weak acid, HA, is shown below. As the titration progresses, HA is…

A: A question based on titration curve, which is to be accomplished.

Q: What is the pH of a buffer made by mixing 0.155M HC2H3O2 with 0.225M NaC2H3O2 to a total volume of…

A: Given: Concentration of weak acid HC2H3O2 = 0.155 M Concentration of NaC2H3O2 = 0.225 M And volume…

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.