Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. Topic: Acid-Base Equilibria and Neutralization Methods Balance Equations a.) Write the Mass Balance Equations for the following solutions: - 0.10 F H2A - 0.20 F NH4Cl b.) Write the Charge Balance Equations for the following solutions: - 0.10 F H2A - 0.20 F NH4Cl
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Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE.
Topic: Acid-Base Equilibria and Neutralization Methods
Balance Equations
a.) Write the Mass Balance Equations for the following solutions:
- 0.10 F H2A
- 0.20 F NH4Cl
b.) Write the Charge Balance Equations for the following solutions:
- 0.10 F H2A
- 0.20 F NH4Cl
c.) Write the Proton Balance Equations for the following solutions:
- H2SO3
- Na2SO3
Step by step
Solved in 2 steps
- What is the pH of the solution after mixing 0.171 g of Mg(OH)2 (MW=58.321 g/mol) with 68.9 mL of 0.0569 M HCl? The resulting solution was diluted to 100 mL. Round your calculated value for pH to two figures to the right of the decimal point.1. The reaction of ??? with ???3 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+ ___ HNO3 (aq) ---> ___ KNO3 (aq)+ ___ H2O(l)Calculate the molar concentration of Nitric acid (???3) when 40.5−?? of 0.674 ? ???is required to quench 101.0?? of Nitric acid over phenolphthalein indicator.A 10.00cm3 portion of the 100.00cm3 HCl solut was taken from the volumetric flask and was titrated with KOH (aq). It was neeutralized by 24.35cm3 of potassium hydroxide od concentration 0.0500moldm-3. Calculate the concentrat of the original concentrated hydrochloric acid in moldm-3.
- Write both the charge balance equation (CBE) and mass balance equation (MBE) for the following solutions at equilibrium: 1. 0.12 M H2A 2. 0.40 M NH4ClA 0.128 g sample of KHP (HKC8H4O4) required 28.54 mL of NaOHsolution to reach a phenolphthalein endpoint. Calculate the molarity of theNaOH.Hint: first balance the acid base reaction of KHP with NaOH.A. 0.110 M NaOHB. 0.0220 M NaOHC. 1.032 M NaOHD. 0.921 M NaOHPlease answer it ALL ASAP and CORRECTLY for an upvote. PROVIDE YOUR FULL SOLUTION. You prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 ml of 0.13 M ammonium chloride. The dissociation constant of ammonia is 1.8x10^-5 What is the total volume of the buffer? What is the final concentration of the base? What is the final concentration of the salt? What is the acid strength of the solution? What is the pH of the buffer solution?
- A 250 cm3 volumetric flask contains exactly 200,0 cm3 of a 0,025 mol.dm3sulphuric acid solution. Thereafter ten (10) sodium hydroxide pellets, eachof mass 0,1 g are dropped into the flask. After the pellets have dissolvedcompletely, the flask is topped to the 250 cm3 mark with water and thecontents are thoroughly homogenised. Determine the pH of the resultingsolution.For water having a total alkalinity of 1.00x10^-3 mol/L and a pH of 10.34 what is the percentage contribution to alkalinity from CO32-? Please answer very soon will give rating surelyIf a titration net volume for the standardization should be 23.50 mL and a student accidentally one drop past the endpoint (~0.05 mL), will the calculated NaOH concentration (M) be higher or lower than the true value of that solution’s concentration? Explain briefly.
- The salt K2HPO4 (potassium hydrogen phosphate) is a strong electrolyte but not a strong acid or base. Consider an F = 0.010 M solution of K2HPO4. a) Add the acid/base behavior of hydrogen phosphate by writing a “sequential dissociation scheme” for phosphoric acid (H3PO4). Then write mass balance equations for total phosphate and total potassium and give their numerical values. b) Write the charge balance equation for this solution. How may total species are there? [Count species in the charge balance equation and add any neutrals.] How many additional equations are needed for systematic treatment of equilibrium? Name them (give their usual symbols) c) Consider the KHPO4−(aq) ion pair. This is a new species, so what additional equation would you need? Tell how you would alter each charge or mass balance equation (if necessary) to include this species.Please answer with complete solutions. Do not use spreadsheet. Thank you A series of solutions containing NaOH, Na2CO3, and NaHCO3, alone or in compatible combination, was titrated with 0.1202 M HCl. Tabulated below are the volumes of acid needed to titrate 25.00-mL portions of each solution to (1) a phenolphthalein and (2) a bromocresol green end point. Use this information to deduce the composition of the solutions. In addition, calculate them molar concentration. (1) Phenolphthalein End Point (2) Bromocresol Green End Point a 22.42 22.44 b 15.67 42.13 c 29.64 36.42 d 16.12 32.23 e 0.00 33.33Please answer with complete solutions. Do not use spreadsheet. Thank you A series of solutions containing NaOH, Na2CO3, and NaHCO3, alone or in compatible combination, was titrated with 0.1202 M HCl. Tabulated below are the volumes of acid needed to titrate 25.00-mL portions of each solution to (1) a phenolphthalein and (2) a bromocresol green end point. Use this information to deduce the composition of the solutions. In addition, calculate the mass in milligrams of each solute per milliliter of solution.