Question

In: Chemistry

find the pH in a mixture of: a) 50 ml 0,10 mol/L HCL and 10 mL...

find the pH in a mixture of:
a) 50 ml 0,10 mol/L HCL and 10 mL 0,50 mol/L NaOH

b) 50 mL 0,10 mol/L HCL and 20 ml 0,50 mol/L NaOH

c) 100 mL 0,20 mol/L CH3COoH and 50 mL 0,20 mol/L NaOH

thx

Solutions

Expert Solution


Related Solutions

1000 mol/min of a mixture of 90 mol% air and 10 mol% HCl enters an absorber...
1000 mol/min of a mixture of 90 mol% air and 10 mol% HCl enters an absorber column and is contacted with a stream of pure water entering the column at the rate 300 moles/min. 90% of HCl in the feed gas is absorbed by water. The two exit streams are gas stream (air+HCl) and liquid stream (water+HCl), respectively. 1. Draw and label a flowchart. 2. Define a basis of calculation. 3. Carry out a degree of freedom analysis and determine...
A 18.6 mL solution of 0.100 mol L-1 NaOH is titrated using 0.150 mol L-1 HCl....
A 18.6 mL solution of 0.100 mol L-1 NaOH is titrated using 0.150 mol L-1 HCl. What is the pH of the solution after 15.3 mL of the HCl solution is added?
Calculate the pH if 0.03 mol HCl is added to 0.500 L of a buffer solution...
Calculate the pH if 0.03 mol HCl is added to 0.500 L of a buffer solution that is 0.24 M NH3 and 0.20 M NH4Cl? For NH3 Kb= 1.8 x 10-5
Calculate the pH after adding 10.00 mL of 0.15 M HCl to 50 mL of the...
Calculate the pH after adding 10.00 mL of 0.15 M HCl to 50 mL of the ammonia/ammonium ion buffer solution with a ph of 4.82
Determine the pH change when 0.093 mol HCl is added to 1.00 L of a buffer...
Determine the pH change when 0.093 mol HCl is added to 1.00 L of a buffer solution that is 0.497 M in HNO2 and 0.311 M in NO2-. pH after addition − pH before addition = pH change = ___________________ Determine the pH change when 0.115 mol KOH is added to 1.00 L of a buffer solution that is 0.457 M in HNO2 and 0.256 M in NO2-. pH after addition − pH before addition = pH change =_____________
A mixture of 0.2063 mol of Cl2, 0.2093 mol of H2O, 0.1887 mol of HCl, and...
A mixture of 0.2063 mol of Cl2, 0.2093 mol of H2O, 0.1887 mol of HCl, and 0.09871 mol of O2 is placed in a 1.0-L steel pressure vessel at 575 K. The following equilibrium is established: 2 Cl2(g) + 2 H2O(g) 4 HCl(g) + 1 O2(g) At equilibrium 0.05821 mol of O2 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Cl2, H2O, HCl, and O2. (b) Calculate KP for this reaction.
A student conducts a titration of 50 mL of HCl with 1.00 M NaOH. The pH...
A student conducts a titration of 50 mL of HCl with 1.00 M NaOH. The pH at the equivalence point is Basic Neutral Acid
find the pH of a 40 mL buffer solution + 1.0 mL of 6.0 M HCl...
find the pH of a 40 mL buffer solution + 1.0 mL of 6.0 M HCl (aq) I know this question is pretty simple, but do I need to know what the buffer is made of? Is it important? if not how would I set up the ICE table? thank you!
HCl: -164.4 kJ/mol NaOH: -469.6 kJ/mol NaCl: -407.1 kJ/mol H2O: -285.9 kJ/mol If 50 mL of...
HCl: -164.4 kJ/mol NaOH: -469.6 kJ/mol NaCl: -407.1 kJ/mol H2O: -285.9 kJ/mol If 50 mL of 1.00 M HCl and 50 mL of 2.00 M NaOH are mixed, given the enthalpies of formation above, use Hess's Law to calculate the molar heat of neutralization.
Find the pH of the following solutions: a mixture of 10.0 mL NaOH solution having pH...
Find the pH of the following solutions: a mixture of 10.0 mL NaOH solution having pH 11.00 and 10.0 mL HClO4 having pH 1.00. 2.) Using activities calcalute the pH and concentration of H+ in pure water containing 0.05 M CaCl2 at 25 degrees C
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT