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How to Edit Your Silver Nitrate Molar Mass Online
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How to Edit Text for Your Silver Nitrate Molar Mass with Adobe DC on Windows
Adobe DC on Windows is a useful tool to edit your file on a PC. This is especially useful when you deal with a lot of work about file edit without using a browser. So, let'get started.
- Click the Adobe DC app on Windows.
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- Click the Select a File button and select a file from you computer.
- Click a text box to adjust the text font, size, and other formats.
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How to Edit Your Silver Nitrate Molar Mass With Adobe Dc on Mac
- Select a file on you computer and Open it with the Adobe DC for Mac.
- Navigate to and click Edit PDF from the right position.
- Edit your form as needed by selecting the tool from the top toolbar.
- Click the Fill & Sign tool and select the Sign icon in the top toolbar to customize your signature in different ways.
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How to Edit your Silver Nitrate Molar Mass from G Suite with CocoDoc
Like using G Suite for your work to complete a form? You can make changes to you form in Google Drive with CocoDoc, so you can fill out your PDF without worrying about the increased workload.
- Go to Google Workspace Marketplace, search and install CocoDoc for Google Drive add-on.
- Go to the Drive, find and right click the form and select Open With.
- Select the CocoDoc PDF option, and allow your Google account to integrate into CocoDoc in the popup windows.
- Choose the PDF Editor option to open the CocoDoc PDF editor.
- Click the tool in the top toolbar to edit your Silver Nitrate Molar Mass on the Target Position, like signing and adding text.
- Click the Download button to save your form.
PDF Editor FAQ
What is the molarity of a solution containing 50.00g of silver nitrate?
You had to provide the volume of the solution to get the molarity of the solution.Molarity = (mass/molar mass) × (1000mL/volume of solution in mL)Hope, this helps.
What is the mass in grams of 3.45x10-2 moles of silver nitrate?
At first glance:Molar mass of AgNO3: 169.8733 g/mol3.45*10^-2 mol * 169.8733 g/mol = 5.86062885 gUnless this is a trick question ?
What is the concentration of a solution of silver nitrate if 50.0 mL of the solution reacting with excess potassium chloride gives 10 g of precipitate?
The reaction involved here is: AgNO3 + KCl = AgCl + KNO3.The white precipitate formed is that of silver chloride, AgCl.Stoichiometrically, 1 mole of AgNO3 gives 1 mole of AgCl on treatment with excess KCl.Amount of AgCl formed = 10 gm = 10/143.5 = 0.07 mole. (Molar mass of AgCl = 143.5 gm)Therefore, amount of AgNO3 needed to form 0.o7 mole (10 gm)of AgCl = 0.07 mole.Now, number of moles of AgNO3 in 50 ml of the solution = 0.07So, number of moles of AgNO3 in 1 litre (1000 ml) = 1000 x 0.07/50 = 1.4.The concentration of the silver nitrate solution is 1.4 M.
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