what is the Ag+]init (M) [C2H3O2-]init (M for flask d e and f ? What is the Moles SCN- used in titration (mol) & Moles of Ag+ in 20.0 mL titrated (mol) for flask d e and f
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what is the
Ag+]init (M)
[C2H3O2-]init (M
for flask d e and f ?
What is the
Moles SCN- used in titration (mol) &
Moles of Ag+ in 20.0 mL titrated (mol)
for flask d e and f
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- Type your numerical answers in the box provided in three significant figures (e.g., 0.123). Do not report your answer in scientific notation. No need for units. If Canvas drops your last zero digit/s, it is OKAY. (e.g. 1.20 to 1.2). Consider a solution of 0.00500 M HBr for numbers 22-24. Determine the following: 22. equilibrium molar concentration of H3O = M. M. 23. equilibrium molar concentration of Br = %3D 24. pH =MISSED THIS? Read Section 18.8 (Pages 829 - 833). Part A A solution is made that is 1.0x10-3 M in Zn(NO,), and 0.130 Min NH3. After the solution reaches equilibrium, what concentration of Zn?+ (aq) remains? Express your answer using two significant figures. Zn]= 5.1• 10- M Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remainingFill in the left side of this equilibrium constant equation for the reaction of dimethylamine ((CH,) NH (CH,),NH). a weak base, with water. 미□
- A 1.00 liter solution contains 0.60 moles nitrous acid and 0.46 moles potassium nitrite .If 0.23 moles of perchloric acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of perchloric acid.) A. The number of moles of HNO2 will increase. B. The number of moles of NO2- will remain the same. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase.Part3: Based on your ICE table and equilibrium expression Kb, determine the initial moles of NaClO added to this solution.II. Math Based Problems: (Show Work! You may write out on paper, scan in as a picture and use the insert signature function in Acrobat Reader DC to insert the picture) Use this equation to answer the following questions. H2PO4 (ag) + H20 (1) +→ H30* (ag) + HPO4 (ag) 1. Tadded 0.005 M solutions of each reactant together. At equilibrium, I found a 0.003 M concentration of HPO4?. (Hint: Does NOT require use of the quadratic equation) A. What is the Ka of my solution? B. What is the pH of my solution at equilibrium?
- What is the value of the equilibrium constant (K) for the following neutralization reaction: ?3?++??−⟶2?2?H3O++OH−⟶2H2O Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Hint: To answer this question, you may need to use the value of Kw stated in the lab manual.Chemistry PART THREE: Carbonate Chemistry 1. A natural lake has a pH of 5.2. In descending order of concentration (highest to lowest), the inorganic carbon speciation (H2CO3, HCO3, CO2) in this lake would be: 2. Find the concentration of moles per liter at equilibrium of carbon dioxide dissolved in water at 20C. The partial pressure of carbon dioxide is 415 x 10-6 atm.Evaluate this statement: A low value for K eq means thatboth the forward and reverse reactions are occurringslowly.
- For the reaction: H₂O(l) 2NH3(g) + CO2(g) = (NH2)2CO(s) + ΔΗ = – 330 kJ == Predict how each of the following changes would impact a reaction that is currently at equilibrium. That is, which way would the reaction progress in order to respond to the change in the system to regain equilibrium (use arrows to show the direction of change that would occur to return back to equilibrium). Explain your reasoning for each part.57. Consider the reaction: MISSED THIS? Read Section 16.8; Watch KCV 16.8, IWE 16.12 HC,H,O;(aq) + H,0(1) = H;O*(aq) + C,H;O, (aq) K = 1.8 x 10 $ at 25 °C If a solution initially contains 0.210 MHC,H;02, what is the equilibrium concentration of H,0*at 25 °C?Determine concentration of hydroxide ion, OH, in a solution of HNO2 by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the concentration of OH-. Complete Parts 1-3 before submitting your answer. NEXT > A 0.60 M aqueous solution of HNO2 is prepared. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) 1 2 3 HNO₂(aq) + H₂O(l) 2 NO₂ (aq) + H3O+ (aq)