suppose you need 50.0 ml of a 1.0 M solution of HCL. What volume of 6.0 M will you use?
suppose you need 50.0 ml of a 1.0 M solution of HCL. What volume of 6.0...
C. Efect of Varving Temperature Constant volume of 6.OM HCl used is 6.0 mL Constant volume of diluted HCl is 50.0 mL Run Number Temperature (oC) Time to Produce 30. ml of H, gas (see) 9.98 20 Run 1 is the same data which was recorded for Run 3 of Part A above. Show all calculations and be sure to include units and the correct number of significant figures. 1. For each dilution of the 6.OM HCI in Part A....
Question 355 pts 50.0 mL of a 3.00 M HCl solution is diluted to a total volume of 276.3 mL. What is the concentration of the diluted solution?
1. A solution (50.0 mL) of 0.125 M HCl is being titrated with 0.125 M KOH. What species are present in this solution, and what is the pH: (a) Before any KOH solution has been added? (b) After 50.0 mL KOH solution has been added? (c) After 25.0 mL KOH has been added? (d) After 75.0 mL KOH has been added? Can all work be shown? Equations/ Ice charts If applicable-please include them. I need to understand. Thank-you in advance.
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed in a constant-pressure calorimeter, the temperature of the solution increases from 21.0°C to 27.5°C. Calculate the enthalpy change of the reaction per mole of HCl assuming the solution has a total volume of 100.0 mL and a density of 1.000 g/mL. The specific heat of water is 4.184 J/q°C Asoln = 2720
reaction one NaOH and HCl. 50.0 mL of 2.0 M HCl solution into 50.0 mL of 2.0 M NaOH reaction two 50 mL OF 2.0 M NaOH into 50 mL of 2.0 M NH4Cl reaction three 50.0 mL of 2.0 M HCl into 50.0 mL NH3 pleanse answer all of the questions Experinen DATA TABLE Reaction 1 Reaction 2 Reaction 3 34,012。21 2H0 Maximum temperature (C) Initial temperature (C) Temperature change (&T) DATA ANALYSIS 1. Calculate the amount of heat...
Calculate the pH of the following solutions: 50.0 mL 0.10 M acetic acid + 1.0 mL 1.0 M HCl 50.0 mL 0.10 M acetic acid + 1.0 mL 1.0 M NaOH 50.0 mL 0.10 M sodium acetate + 1.0 mL 1.0 M HCl 50.0 mL 0.10 M sodium acetate + 1.0 mL 1.0 M NaOH 50.0 mL 0.10 M acetic acid/sodium acetate buffer 50.0 mL 0.10 M acetic acid/sodium acetate buffer + 1.0 mL 1.0 M HCl 50.0 mL 0.10...
A 50.0 mL solution of 0.150 M KOH is titrated with 0.300 M HCl. Calculate the pH of the solution after the addition of the following amounts of HCl. d) 18.0 mL HCl e) 24.0 mL HCl g) 26.0 mL HCl h) 29.0 mL HCl
To what volume should you dilute 35 mL of a 13 M stock HCl solution to obtain a 0.580 M HCl solution?
A solution of HCl is prepared by diluting 25.0 mL of a 1.0 M HCl solution with enough water to make 750 mL of HCl solution. (Show your work for all calculations!) a) What is the molarity of the HCl solution? b) What is the [H3O+] and the pH of the HCl solution? c) Write the balanced chemical equation for the reaction of HCl and Ba(OH)2 d) How many milliliters of the diluted HCl solution is required to completely react...
2. Calculate the pH of a solution prepared by diluting 0.25 mL of a 6.0 M HC red by diluting 0.25 mL of a 6.0 M HCl with water to a total 1.25 ml. Record this pH in Part I data sheet, Beaker #1 for Theoretical Final pH. 3. Calculate the pH of a solution prepared by dilutine 0.25 mL of a 6.0 M NaOH with water to a total volume of 20.25 mL. Record this pH in Part I...