Titration Curves pH versus mL of 0.09795 M NaOH First Determination Hd 14 12 10 00 8 6 4 2 0 0.0204.06.08.00.00.00.16.08.20.20.20.26.28.80.80.80.80.38.40.40.00.46.48.50.50.50.00 mL of NaOH

Part A Classify each of the following as ionic or molecular. Drag the appropriate items to their respective bins. MgCO3 FePO3 AsCl3 N₂O3 Ba3(PO4)2 Al(ClO2)3 Co(C₂H3O2)2 lonic Submit Request Answer Reset Help Molecular

How are the two BRs related and how are the OH figures related

a. Rubidum chloride, RbCl, and sulfuric acid, H₂SO4 Rule 4: an exception to the rule for sulfates; RbCl(aq) + H₂SO4 (aq) → Rb₂SO4(s) + HCl(aq) Rule 4: an exception to the rule for sulfates; 2RbCl(aq) + H₂SO4 (aq) → Rb₂SO4 (8) + 2HCl(aq) Rule 4: an exception to the rule for sulfates; 2RbCl(aq) + H₂SO4 (aq) → Rb2SO4 (aq) + 2HCl(aq) O No precipitate: both Rb₂SO4 and HCI are soluble RbCl(aq) + H₂SO4 (aq) → no precipitate b. Potassium carbonate, K₂CO3, and barium chloride, BaCl₂ O Rule 6: Most carbonate salts are only slightly soluble; K₂CO3(aq) + BaCl₂ (aq) → BaCO3(s) + 2KCl(aq) O Rule 6: exeption to rule for carbonates; 2K₂CO3(aq) + BaCl₂ (aq) → BaCO3(s) + 2KCl(aq) O Rule 6: Most carbonate salts are only slightly soluble; K₂CO3(aq) + BaCl₂ (aq) → BaCO3(aq) + 2KCl(aq) O Rule 6: Most carbonate salts are only slightly soluble; K₂CO3(aq) + BaCl2 (aq) → BaCO3 (8) + KCl(aq) c. Sodium sulfate, Na2SO4, and barium nitrate, Ba(NO3)2 O Rule 4: an exception to the rule for sulfates; Na₂SO4 (aq) +…

Acetic acid has a Ka value of 1.8×105, what is its Kb value? Section а. 5.6×10-10 b. 1.8×10-19 c. 5.6×10-5 d. 1.8×10° С. Section

help me please

(d) For the following reaction: OH Na O a. draw the products and label the acid, base, conjugate acid and conjugate base with pk, values b. show your work for calculating the Kea of the reaction in the forward direction

Solve correctly please. (Gpt/Ai wrong answer not allowed)

Calculate the pką of an acid with Ka = 7.77 x 10-4. %3D O A. 2.230 О в. 3.110 O C. 4.147 D. 7.160 O E. 10.089

Shop Trendy CHEM 1032Cengage S19 34 https://ng.cengage.com/static/nb/ui/evo/index.html?elSBN-9781305657571 &id-430934266&isnapshotld-10652508 s19 3.4 Cengage MInbox (112) DTAP Q Search this course L ions Use the References to access important values if needed for this question. The rate constant of the elementary reaction H2(g) +Br2(g) 2HBr(g) is k 4.45x10 L mol s at 250°C, and the reaction has an activation energy of 170 kJ mol (a) Compute the rate constant of the reaction at a temperature of 289°C L mol , 1 (b) After e (b) After equal concentrations of H, and Bry are mixed at 250o C, 6,03 10' s is required for half of them to be consumed. How long will itke to consume half of the reactants if an identical experiment is performed at 289°C? Submit Answer 3 question attempts remaining Autosaved at 9:31 AM Back 9:31 2/28