15.27a | Calculate the concentrations of ions in a saturated solution of AgI

(4:30)

15.27a | Calculate the concentrations of ions in a saturated solution of AgI

(1:18)

15.27d | Calculate the concentrations of ions in a saturated solution of Sr(OH)2·8H2O

(8:16)

15.27b | Calculate the concentrations of ions in a saturated solution of Ag2SO4

(8:2)

WS17 Q11

(7:38)

15.27c | Calculate the concentrations of ions in a saturated solution of Mn(OH)2

(8:2)

15.28a | Calculate the Ksp for AgBr: [Ag+] = 5.7 × 10–7 M, [Br–] = 5.7 × 10–7 M

(4:1econd)

15.13a | Calculate the molar solubility of KHC4H4O6 from its solubility product

(6:23)

15.48 | The calcium ions in human blood serum are necessary for coagulation (Figure 15.5). Potassium

(24:31)

15.95 | What is the molar solubility of BaSO4 in a 0.250-M solution of NaHSO4? Ka for HSO4−

(17:17)

15.21 | Refer to Appendix J for solubility products for calcium salts. Determine which of the

(19:21)

Calculate the pH of a solution that is made when 0.250 L of 0.20 M benzoic acid (pKa=4.20) and 2.30g

(6:37)

15.16c | Calculate the concentration of all solute species: Ag2CrO4(s) in 0.225 L of a solution

(15:15)

15.31c | How to find if a compound precipitates from a solution: CaHPO4

(5:3)

15.74 | A roll of 35-mm black and white photographic film contains about 0.27 g of unexposed AgBr

(19:25)

15.51 | Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the

(27:20)

15.31d | How to find if a compound precipitates from a solution: Pb3(PO4)2

(5:53)

15.23 | Public Health Service standards for drinking water set a maximum of 250 mg/L (2.60 × 10–3 M)

(7:8)

15.10a | Calculate the solubility product for BaSiF6, 0.026 g/100 mL (contains SiF6 2− ions)

(9:21)

15.14a | Calculate the molar solubility of Ag2SO4 from its solubility product

(7:55)

15.24a | Calculate [Ag+] in a saturated aqueous solution of AgBr

(4:40)

15.17b | Calculate the concentration of all solute species: BaF2(s) in 0.0313 M KF

(16:13)

N-Gen Math Algebra I.Unit 6.Lesson 1.Exponential Increase and Decrease

(34:54)

15.24b | What will [Ag+] be when enough KBr has been added to make [Br–] = 0.050 M?

(5:51)

15.28c | Calculate the Ksp for PbF2: [Pb2+] = 2.1 × 10–3 M, [F–] = 4.2 × 10–3 M

(4:15)

15.11a | Calculate the solubility product for BaSeO4, 0.0118 g/100 mL

(10:5)

15.33 | Calculate the concentration of sulfate ion when BaSO4 just begins to precipitate from a

(5:28)

15.26a | Calculate the concentrations of ions in a saturated solution of TlCl

(4:29)

2023 HIGH INTEREST RATES!! Home Affordability Rule/Calculation

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