When a 1.00 M NaCl solution (aqueous) is interfaced with a 3.5 M KCl solution (aqueous), a liquid junction potential (magnitude) of 1.9 mV is measured at 25^{o}C. Using a well-labeled figure, show and explain how the liquid junction potential occurs.
When a 1.00 M NaCl solution (aqueous) is interfaced with a 3.5 M KCl solution (aqueous),...
When a 1.00 M NaCl solution (aqueous) is interfaced with a 3.5 M KCl solution (aqueous), a liquid junction potential (magnitude) of 1.9 mV is measured at 25oC. Using a well-labeled figure, show and explain how the liquid junction potential occurs.
What is the freezing point of an aqueous 1.00 m NaCl solution? (Kf = 1.86 *C/m) (Assume complete dissociation of the salt.) I know the answer is -3.78*C but I cannot figure out how to get it. I keep getting -1.86*C. Please show step by step so I can understand. Thank you.
A. Calculate the ionic strength of an aqueous solution of 0.037 M KCl. B. How will the activity of 0.025 M Ca2+ be impacted by the addition of 0.050 M KCl? In other words will the activity of Ca2+ increase or decrease when KCl is added to pure water? Briefly explain your answer.
QUESTION 10 Observed liquid junction potential for 0.1 M HCI 0.1 M KCI is +27 mV, while junction potential for the same concentration of 0.1 M NaCl 0.1 M KCI is -6.4 mV, select the correct statement from the following A. Junction potential is a measurement of how fast e-are transferred through the interface B. the opposite sign of the two junction potentials suggest the opposite flow of ions C. electrons transfer faster for the 0.1 M HCI 10.1 M...
Consider an aqueous solution comprised of 0.150 M NH3 and 0.200 M NH4Cl. The pKb of NH3 is 4.75 and the volume of the solution is 1.00 L. a) What is the pH of this solution? Show your work. b) What is the chemical reaction (balanced chemical equation) that occurs when NaOH solution is added to the original solution? c) How many moles of NaOH(s) could this solution react with before its pH rises to 10.00? Show your work.
An aqueous NaCl solution is made using 126 g ofNaCl diluted to a total solution volume of 1.00 L . Calculate the molarity of the solution. Express your answer using three significant figures. M = 2.16 M Part B Calculate the molality of the solution. (Assume a density of 1.08 g/mL for the solution.) Express your answer using two significant figures. m = 2.3 m Part C Calculate the mass percent of the solution. (Assume a density of 1.08 g/mL...
2. Consider an aqueous solution comprised of 0.200 M NH3 and 0.150 M NHACI. The pKb of NH3 is 4.75 and the volume of the solution is 1.00 L. a) (2 marks) What is the pH of this solution? Show your work. b) (1 mark) What is the chemical reaction (balanced chemical equation) that occurs when NaOH solution is added to the original solution? c) (3 marks) How many moles of NaOH(s) could this solution react with before its pH...
4. When Ca metal is placed in an aqueous solution of NaCl, the calcium slowly disappears and bubbles form. A litmus test shows that the solution turns basic. Is this evidence that Cais more active than Na? Explain briefly!
What is the molality of NaCl (58.5 g/mol) in an aqueous solution which is 4.2 molar? The density of the solution is 1.05 g/mL. ANSWER: 5.22 m Please, show the steps using dimensional analysis if possible. Thank you
Please I need help with number 54 and 61 please An aqueous NaCl solution is made using 112 g of NaCl diluted to a total solution volume of 1.00 L. Calculate the molarity, molality, and mass percent of the solution. (Assume a density of 1 08 g/mL for the solution.) An aqueous KNO_3 solution is made using 72.5 g of KNO_3 diluted to a total solution volume of 2.00 L. Calculate the molarity, molality, and mass percent of the solution....