sing the constant below, calculate the molar concentration (M) of acid H30+ in olution if the concentration of OH- is 3.4 x 10-5. Kw = 1.0 x 1014 M²= [H3O*][OH¨] %3D O a) 2.9 x 10 10 O b) 2.0 x 1010 O c) 3.4 x 10-9 O d) 2.4 x 10-10 O e) 3.4 x 109
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![Using the constant below, calculate the molar concentration (M) of acid H3O* in
solution if the concentration of OH- is 3.4 x 10-5.
Kw = 1.0 × 10-14 M²= [H3O*][OH].
%3D
O a) 2.9 x 10-10
O b) 2.0 x 10-10
O) 3,4 x 109
d) 2.4 x 10-10
e) 3.4 x 109](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F735b0976-906f-40ec-a76b-1f1d9f7b453e%2Fc3c5d7e0-a4f1-4fbc-a901-96c33cac890e%2Ff6lav6_processed.jpeg&w=3840&q=75)
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- Which of the following is (are) NOT true for a solution at 25°C that has a hydroxide ion concentration, [OH-] = 2.5 x 10-6 M? L × O the ]H+] = 4.0 × 10-⁹ M the Kw is independent of what the solution contains OK₂ = 1 x 10-14 O The solution is acidic O the ]H+] = 4.0 × 10-8 M the solutin is basicStrong Acids; Calculate pH [HA]o [H;O"] pH Step 1 Calculate [H3O] based on the fact that strong acids react completely with water. Step 2 Calculate the pH using the equation: pH = -log (H;O"] What is the pH of a 1.73×10 M solution of the strong acid HC10,? HCIO,(aq) + H20(1) → C10, (aq) + H3o*(aq) [HC10], = 1.73×10-5 SubmitAt 25°C, what are the molar H3ot and OH concentrations in a 0.0360 M CG H; COOH (K, (C,H; COOH)= 6.28 x 10)? M %3D [OH ]- %3D M bo.0360 M HN3 (K, (HN3)= 2.2 x 10 )? 1--HO] C0.240 M hydroxylamine hydrochloride (K, (NH,OH)= 9.09 x 10 )? [1,0*] -[ (OH |-
- Calculate the concentration for the following pH: pH = 7.00 (A) (H:0*] = 1 x 10-9 M (B) (H30*] = 1 x 10-7 M (C) (H304] = 2x 107 M (D) (H30*] = 1 x 10-3 M 34Help Asha balance the following equation by completing the equation with the correct numbers: _P4+_F2› PF3 35.Asha balance the following equation by completing the equation with the correct numbers: _H2 + _F2>HF can you help me with these last 3... please . I don't understand it. Calculate the moles of H+ delivered to eachsample based on your experimental dataand record these values in Data Table 2. 0.1M HCl = 0.1 moles HCl / 1 Liter solutionCalculate the moles of OH- in each sampleand record these values in Data Table 2. H+ + OH- H2O Calculate the moles of Ca2+ in each sampleand record these values in Data Table 2. Ca(OH)2 Ca2+ + 2OH24. Calculate the molar solubility of Ca(OH)2for each sample and record these values inData Table 1. Molar solubility = moles / Liter Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.37 25.37 25.37 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.18 28.21 28.28 Mass of Calcium Hydroxide Solution Volume of Ca(OH)2 Density = 1.000 g/mL Concentration of HCl (M) Initial HCl volume in Syringe 1.0ml 1.0ml 1.0ml Final HCl volume in Syringe .54ml .58ml .5ml Volume of HCl Delivered .46ml .42ml…Calculate the moles of H+ delivered to eachsample based on your experimental dataand record these values in Data Table 1. 0.1M HCl = 0.1 moles HCl / 1 Liter solution Calculate the moles of OH- in each sampleand record these values in Data Table 1. H+ + OH- H2O Calculate the moles of Ca2+ in each sampleand record these values in Data Table 1. Ca(OH)2 Ca2+ + 2OH . Calculate the molar solubility of Ca(OH)2for each sample and record these values inData Table 1. Molar solubility = moles / Liter . Calculate the Ksp for each trial and theaverage Ksp and record these values inData Table 1. Ksp = [Ca2+][OH-]2 Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.47 25.47 25.47 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.32 28.30 28.43 Mass of Calcium Hydroxide Solution 2.85 2.83 2.96 Volume of Ca(OH)2 Density = 1.000 g/mL Concentration of HCl (M) Initial HCl Volume in Syringe 1.0ml…
- Strong Acids; Calculate pH [HA]o [H;O"] pH Step 1 Calculate [H30"] based on the fact that strong acids react completely with water. Step 2 Calculate the pH using the equation: pH = -log [H;O¯] What is the pH of a 1.73×10M solution of the strong acid HCIO,? HCIO,(aq) + H2O(t) → C10,(aq) + H30*(aq) [HCIO4]0 = 1.73×10-5 Submit What is the concentration of hydronium ion following reaction between the acid and water? Submit Calculate the pH of the solution based on the solution to the previous question (shown below). [H;O*] = 1.73x10-5 MD Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. Note: Solution 1 (Choose one) 2 = H₂O Explanation Solution 3 (Choose one) ▼ W S ▼ Check 3 747 E D (Choose one) Solution 2 $ (Choose one) 4 Solution 4 R % 5 T X 80 G 6 3 MacBook Pro Y & 7 H © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A U 8 J 1 ( 9 ➡ K ) O O P OConsider the following chemical equilibrium for the weak base CN in water: CN- (aq) + H₂O(1) = HCN (aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d pH will go up; [OH-] will go up; net amount of OH will go up pH will go down; [OH-]will go up; net amount of OH will go down pH will go down; [OH-]will go down; net amount of OH will go down pH will go up; [OH-] will go up; net amount of OH will go down
- At 100o C, Kw = 4.9 x 10-13 . What is the pH of a solution at 100o C if [OH-] = 6.3 x 10-12The pH Scale [H;O"] pH pOH [OH'] Step 1 Calculate the solution's pH using the equation: pH = -log[H;0*] Step 2 Determine the value of pOH using the equality: pH + pOH = pKw; at 25 °C, pKw = 14.00, so pH + pOH = 14.00 Step 3 Calculate [OH] using the equation: pOH = -log[OH] At 25 °C, a solution has a hydronium ion concentration of 3.20×10-8 M. What is the pH, pOH, and [OH] of this solution? pH = | pOH %3D [OH']=| M SubmitEach value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral Answer Bank H]= 1.0 x 10 pll=346 pOl - 541 OH |-26 x 10 pOll =831 pOll = 7.00 o|=98 x 10 " 1-63x 10 pll=10.38 I= 74 x 10 contectua help privecy polisy terma of uas