Additional Questions 1. Another experiment finds that the concentration of Au?+ ions is 6.3 x 10-...
Copper() ions in aqueous solution react with NH3(aq) according to K, -6.3 x 10 Calculate the solubility (in g L) of CuBr(s) (Ks 6.3x 10-9) in 0.54 M NHs(aq). Number g/ L
Copper(1) ions in aqueous solution react with NH,(aq) according to Cu (aq) + 2NH, (aq) — Cu(NH) (aq) K = 6.3 x 100 Calculate the solubility (in g.L-') of CuBr(s) (Kp = 6.3 x 10-) in 0.10 M NH, (aq). solubility of CuBr(s):
Copper(l) ions in aqueous solution react with NH3(aq) according to Cu(NH3);(aq) 10 Cu"(aq) +2NH3(aq) -> K,=6.3 x 10 Calculate the solubility (in g. L-1) of CuBr(s) (Ksp = 6.3x10-9) in 0.64 M NH3(aq). Number g/L
Calculate the concentration of H3O for an aqueous solution with a pH of 6.20. A) 6.3 x 10-7 M E) 4.0 x 10 M 1. B) 1.6 x 10 M C) 1.0x 10-14 M D) 6.20 x 1014 M 2. The pH of a 0.010 M aqueous solution of Ca(OH)2 is A) 11.70 B) 12.00 C) 12.30 E) 1.70 D) 12.60 alution with a nH of 9.60. for an aqueous solution with a pH of 9.60. C) 1.5 x 10-5...
Calculate the concentration of all species in a 0.14 M KF solution. Ka(HF)=6.3×10−4 Express your answer using two significant figures. Enter your answers numerically separated by commas. Calculate the concentration of all species in a 0.14 MKF solution. K. (HF) = 6.3 x 10 4 Express your answer using two significant figures. Enter your answers numerically separated by commas. PO ALV x x 8 O a ? x x-10 x x x = K+], F-), HF), [OH], H30+] = M...
please answer both questions QUESTION 20 The concentration of H30 in a solution is 7 x 10 Mat 25 °C. What is its hydroxide ion concentration? а. 1 x 10-10 M b. 3x 10-10 м 2* 10 10 M d. 1 x 10-1 M X 7x 104 M QUESTION 21 A solution is 0.012 Min Pb(NO3)2 and 0.20 Min Sr(NO3)2. Solid Na2SO4 is added until a precipitate just begins to form. The and the concentration of sulfate ion at this...
A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x 103 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2 is 1.40 x 10 M. 1. What is the initial concentration in solution of the Fe3 and SCN'? What is the equilibrium constant for the reaction? What happened to the K' and the NO3 ions in this solution? a. b. C. A student mixes 5.12 mL of 4.02 x 10...
Pre-lab Questions for Experiment #11 1) Will a precipitate form when 0.150 L of 0.10 M PHNO The K, for Polis 1.2 x 10-)(Show your calculatio) . 100 L 0,30 M N e w Lof 1 2) Calculate whether a precipitate will form if 2.00 mL of 60 M N aredided to (Show your calculations) -1.8 x 10 and K [FeOH) - 1610) INH! 10 0 4 (Given that N oir 3) Solid silver chromate is added to pure water...
1&2 please! Question 1 Based on the ion-product constant (Kw), calculate the concentration of H+ ions if the concentration of OH-ions is 3.5 x 10^(-4) M. (1 point)* O 2.86 x 10^(-11) M O 3.5 x 10^(-4) M O 3.5 x 10^(10) M O None of the above Question 2 Based on the ion-product constant, calculate the concentration of OH-ions if the concentration of H+ ions in a given solution is 2.67 x 10^(-5) M. (1 point) 0 2.67 x...
Post-lab Questions 1. Ca n you titrate a solution of unknown concentration with another solution of unknown concentrat and still get a meaningful answer? Explain your answer in a few sentences 2. Explain the difference between an end point and equivalence point in a titration. 3. What is the pKa of phenolphthalein? Why is it acceptable to use an indicator whose pKa is not exactly the pH at the equivalence point? 4. What was the concentration of the NaOH solution...