Why does the second drop of 0.1M HCl added to 0.1M NaCl change the PH less than the first drp of 0.1M HCl?
when we add second drop of HCl concentration of HCL in the solution will increase so that H+ increase in the solution.
more the H+ in the solution lesser the pH .
Why does the second drop of 0.1M HCl added to 0.1M NaCl change the PH less...
If 5 mL of 0.1M HCl is added to 50 mL of 0.1M sodium phosphate buffer at pH 7.0, what is the resulting pH?
why does a precipitate form when a drop of 0.6 M HCL is added to a solution of 0.1 M potassium iodide and 0.2 M potassium iodate?
A drop of blood is added to a 1mL solution containing both 0.1M Sucrose and 0.1M NaCl. What is the expected osmolarity of the solution compared to the intracellular fluid of the RBC BEFORE and AFTER the blood is added, respectively? Apply the concept based on the results observed in the lab experiment. (1 pt) Select one: a. hyperosmotic, hypoosmotic b. isoosmotic, hypoosmotic c. hypoosmotic, hyperosmotic d. isoosmotic, isoosmotic e. hypoosmotic, hypoosmotic f. isoosmotic, hyperosmotic g. hyperosmotic,...
Results: As we added 14 drops of 0.1M NaOH to 15 drops of 0.1M HCl and 1 drop of BTB, we have the solution turned to blue. Question: What makes us verify that the reaction is happening? and What is the reaction stoichiometry according to the experimental data? Is this reasonable?
pKa of NH4+ is 5.62*10^-10 what is the pH of solution of 0.1M NH4Cl 40m added to 0.1M HCl 20mL?
What is the pH change when 4.0 mL of 1.0 M HCl is added to 100.0 mL of a solution that is 0.20 M NaH2PO4 and 0.20 M Na2HPO4?Determine the pH when 9.0 mL of 0.80 M NaOH is then added to the results of the first part.
Determine the pH change when 0.068 mol HCl is added to 1.00 L of a buffer solution that is 0.438 M in HF and 0.237 M in F-. pH after addition − pH before addition = pH change = _____________
10) A. Determine the pH change when 0.079 mol HCl is added to 1.00 L of a buffer solution that is 0.466 M in HClO and 0.364 M in ClO-. pH after addition − pH before addition = pH change = B. A buffer solution contains 0.419 M NaHCO3 and 0.285 M K2CO3. Determine the pH change when 0.102 mol KOH is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change =
the first drop down blank says "greater" or "less" the second drop down says "will" or "will not" Will a precipitate form when 100.0 mL of 5.6 x 10M Mg(NO3), is added to 100.0 mL of 8.0 x 10-6 Mi NaOH The ion product for Mg(OH), is Since Q is than Kp, Mg(OH)2 precipitate from the solution. Submit Answer Try Another Version 6 item attempts remaining
a)Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer solution that is prepared by dissolving 4.92g of sodium acetate(molar mass = 82.03gmol^-1) in 250 ml of 0.150 mol L^-1 of acetic acid solution? Assume no change in volume upon addition of either the sodium acetate or HCl. (Ka for acetic acid = 1.8*10^-5) b)Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer...